B. The unbalanced chemical equation for this reaction is given below: NH3(g) + Na(s) --> NaNH2(s) + H2(g) Assuming, Nitrogen gas and hydrogen gas react to form ammonia according to the following thermochemical equation. After the products return to STP, how many grams of nitrogen monoxide are present? Consider the reaction of hydrogen gas with nitrogen gas-producing ammonia, NH_3. What volume (in liters) of ammonia at 15 C an, Methane (CH4), ammonia(NH3), and oxygen(O2) can react to form hydrogen cyanide (HCN) and water according to this equation: CH4 + NH3 + O2 rightarrow HCN + H2O. Write a balanced chemical equation for this reaction. For the CO if you were to use it up completely you would use up 12.7 mols of CO. You need twice as much H2 as CO since their stoichiometric ratio is 1:2. Could oxidation to #NO_2(g)# occur? The combustion of ammonia (a gas) is represented by the equation: 4NH_3 + 5O_2 \to 4NO + 6H_2O How many moles of H_2O (water) is produced when 400g of NH_3 are completely reacted with oxygen? Hydrogen gas and nitrogen gas react to produce ammonia. Ammonia (NH3) reacts with oxygen (O2) to form air pollutant nitrogen oxide (NO) and water. What is Avogadro's law? How can I balance this equation? Write the equation? Ammonia, NH_3, may react with oxygen to form nitrogen gas and water ? not none of these Calculate the molecules of oxygen required to react with 38.8 g of sulfur in the reaction below. Ammonia (NH3) react with oxygen (O2) to produce nitrogen monoxide (NO) and water (H2O). Nitrogen monoxide reacts with hydrogen gas to form nitrogen gas and water (vapor). Hydroperoxyl. When 1.20 moles of ammonia reacts, the total number of moles of products formed is: ? Ammonia NH3 chemically reacts with oxygen gas O_2 to produce nitric oxide NOand water H_2O. 4NH3 + 5O2----4NO + 6H2O All rights reserved. Write the equation for this decomposition. Calculate the number of grams of ammonia needed to form 40.12 moles of nitrogen monoxide. When ammonia (NH_3^(2-)) reacts with dinitrogen oxide (N_2O), the products of the reaction are H_2O(l) and nitrogen gas. If 45.7 g of NH3 and excess of O2 react together, how many grams of NO must be produced to have an 85% yield? d. Gaseous ammonia (NH3) reacts with gaseous oxygen to form gaseous nitrogen monoxide and gaseous water. Ammonia is prepared byreacting nitrogen and hydrogen gases at high temperature accordingto the unbalanced chemical equation shown. A Computer Science portal for geeks. {/eq} reacts with oxygen {eq}(O_2) Scale it down to 2 L O2. What mass of nitric oxide could be produced if 68.0 g of ammonia is mixed with 35.0g of. At constant temperature and pressure, how many liters of ammonia will be formed when 6.00 L of nitrogen reacts with 30.0 L of hydrogen? How many liters of NO are produced when 2.0 liters of oxygen reacts with ammonia? a. Determine the theoretical yield of NO if 21.1 g NH3 is reacted with 42.2 g O2. Gaseous dinitrogen tetroxide (N2O4) decomposes to form nitrogen dioxide gas (NO2). Nitric acid is a component of acid rain that forms when gaseous nitrogen dioxide pollutant reacts with gaseous oxygen and liquid water to form aqueous nitric acid. The mechanism is believed to be 2NO to N_2O_2 N_2O_2 + H_2 to N_2O + H_2O N_2O + H_2 to N_2 + H_2O For this reaction find the following: a) the overall balanced equation. a. 4NH3 + 5O2 --> 4NO + 6H2O Ammonia and oxygen produce nitrogen dioxide and water. What volume of nitrogen monoxide would be produced by this reaction if \( 1.03 \mathrm{~cm}^{3} \) of ammonia were consumed? Hydrogen reacts with nitrogen to produce ammonia: 3H2(g) + N2(g) ---> 2NH3(g). Be sure to balance the reaction using the lowest whole numbers. Understand how to balance chemical equations, practice balancing chemical equations, and see examples. Write the balanced equation for the reaction of nitrogen gas with hydrogen gas to form ammonia gas. Nitrogen monoxide can be prepared by the oxidation of ammonia by the following equation: 4NH3 (g) + 5O2 (g) > 4NO (g) + 6H2O (g). If 15.0 L of nitrogen is formed at STP, how many liters of hydrogen will be produced at STP? N_2 + O_2 rightarrow NO (b) Then. Createyouraccount. we burn 12.50L of ammonia in 20.00L of oxygen at 500 degrees celsius. What is the percentage yield of the reaction? Question: Ammonia gas and oxygen gas react to form water vapor and nitrogen monoxide gas. Write a balanced chemical equation for this reaction. Write and balance the chemical equation. 40.0 g of nitrogen is reacted with 10.0 g of hydrogen. This problem asks how much of a product is produced. Ammonia and oxygen combine to form nitrogen monoxide and water by the chemical reaction: 4 N H 3 ( g ) + 5 O 2 ( g ) 4 N O ( g ) + 6 H 2 O ( l ) If 100 grams of . Furthermore, you can tell from the coefficients in the balanced equation this reaction requires 4 mol of ammonia for every 5 mol of oxygen gas. Ammonia is allowed to react with diatomic oxygen to form nitric oxide and water. 1 Each nitrogen atom is oxidised. In this example, let's start with ammonia:

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The calculation reveals that you'd need 235 g of oxygen gas to completely react with 100 g of ammonia. question: What volume of NH3 is needed to react with 71.6 liters of oxygen. How many grams of oxygen do you need to react with 21.4 g ammonia? Write the chemical equation for the detonation reaction of this explosive. (a) reaction of gaseous ammonia with gaseous HCl (b) reaction of aqueous ammonia with aqueous HCl. 33 Ammonia and chlorine react as shown. Gaseous ammonia chemically reacts with oxygen O2 gas to produce nitrogen monoxide gas and water vapor. 637.2 g of ammonia are reacted with 787.3 g of carbon dioxide. Nitrogen gas and hydrogen gas react to form ammonia according to the following thermochemical equation: 3H2 + N2 arrow 2NH3; Delta H = -96 kJ Write the balanced chemical equation for a reaction involving these substances with the following change in entha, Convert the following into a balanced equation: When nitrogen dioxide is bubbled into water, a solution of nitric acid forms and gaseous nitrogen monoxide is released. Write the balanced equation for the reaction of gaseous ammonia with sulfuric acid solution. Write the. Nitrogen monoxide can be formed according to the equation: N_2 (g) + 2O_2 (g) to 2 NO_2 (g) If 8.0 L of nitrogen is reacted at STP, exactly how many liters of oxygen at STP would be needed to allow complete reaction? This species plays an important role in the atmosphere and as a reactive oxygen . Consider the reaction at 25 degrees Celsius of hydrogen cyanide gas and oxygen gas reacting to form water, carbon dioxide, and nitrogen gases. 6134 views What is the equation for: Gaseous ammonia reacts with gaseous oxygen to form gaseous nitrogen monoxide and gaseous water? Science. If the total pressure of the gas at the end of the rea. Urea (NH_2)_2CO is prepared by reacting ammonia with carbon dioxide. Ammonia and oxygen without catalyst | NH 3 + O 2 N 2 + H 2 O. Peter J. Mikulecky, PhD, teaches biology and chemistry at Fusion Learning Center and Fusion Academy. Sodium Hydrogen Sulfite reacts with hydrochloric acid to produce sulfur dioxide gas, water and sodium chloride NaHSO3 + HCl -----> SO2 + H2O + NaCl 2. Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3NO_2(g)+H_2O(l) to 2HNO_3(l)+NO(g) Suppose that 4.3 mol NO_2 and 0.80 mol H_2O combine and react completely. How many liters of nitrogen will be produced at STP? The balanced chemical equation for the reaction between hydrogen and oxygen to produce water is: 2H2 + O2 -> 2H2O To determine the limiting reactant, we need to compare the amount of hydrogen and oxygen in the mixture to the stoichiometric ratio in the balanced equation. Step 2 - find the molar ratio. Stoichiometry : the numerical relationship between chemical quantities in a balanced chemical equation. How many grams of sodium are needed to produce 2.24 L of hyrdogen collected at 23 and 92.5 kPa? {/eq}. You can ask a new question or browse more stoichiometry questions. Given the equation N2(g) + 3H2(g) = 2NH3(g) determine how many moles of NH3 are produced when 1.4 mol of H2 reacts?Ammonia is produced by the reaction of hydrogen and nitrogen. How can I balance this chemical equations? 3 Ammonia behaves as a base. How many liters of ammonia gas can be formed from 17.2 L of hydrogen gas at 93.0^oC and a pressure of 45.8 kPa? When 34 g of ammonia reacts with 96 g of oxygen, what is the partial pressure of the nitrogen monoxide? What volume of nitrogen monoxide would be . How many grams of ammonia are formed from the reaction of 125.0 grams of nitrogen? Nitrogen dioxide reacts with water to produce oxygen and ammonia: 4NO2 (g)+6H2O (g)7O2 (g)+4NH3 (g) How many grams of NH3 can be produced when 4.10 L of NO2 reacts at 385 C and 735 mmHg ? Show all work! The reactant that is used up is the limiting reagent.\r\n\r\nChemists need to know which reactant will run out first, because that information allows them to deduce how much product and excess reagent they can expect, based on how much of the limiting reagent they've put into the reaction.\r\n

In any chemical reaction, you can simply pick one reagent as a candidate for the limiting reagent, calculate how many moles of that reagent you have, and then calculate how many grams of the other reagent you'd need to react both to completion. How many moles of ammonia gas can be formed from the complete reaction of 44.8 liters of nitrogen gas at standard temperature and pressure (STP), according to the balanced equation, N_2 (g) + 3H_2 (g), Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3 NO_2 (g)+ H_2O (l) to 2HNO_3 (l) + NO (g). Solid ammonium nitrite decomposes to produce gaseous nitrogen and water vapor. With supply of heat, ammonia reacts with oxygen and produce nitrogen gas and water as products. Find out the mass of hydrogen chloride gas needed to react completely with 0.20 g of ammonia gas. How many ammonia liters of ammonia gas is produced when 85 grams of liquid nitrogen completely react? If you are able. But you have only 100 g of oxygen. The one that isn't in excess is the limiting reagent. 4. This allows you to see which reactant runs out first. Gaseous ammonia chemically reacts with oxygen O_2 gas to produce nitrogen monoxide gas and water vapor. (b) How many hydrogen molecules are r, Write out a balanced formula unit equation for the given redox reaction. Potassium metal and chlorine gas combine to form How many types of chemical reactions exist? Use this chemical equation to answer the following questions: 1) Write a balanced equation, including physical state for the reverse reaction. {"appState":{"pageLoadApiCallsStatus":true},"articleState":{"article":{"headers":{"creationTime":"2016-03-26T07:53:28+00:00","modifiedTime":"2021-07-15T14:41:28+00:00","timestamp":"2022-09-14T18:18:26+00:00"},"data":{"breadcrumbs":[{"name":"Academics & The Arts","_links":{"self":"https://dummies-api.dummies.com/v2/categories/33662"},"slug":"academics-the-arts","categoryId":33662},{"name":"Science","_links":{"self":"https://dummies-api.dummies.com/v2/categories/33756"},"slug":"science","categoryId":33756},{"name":"Chemistry","_links":{"self":"https://dummies-api.dummies.com/v2/categories/33762"},"slug":"chemistry","categoryId":33762}],"title":"Calculate Limiting Reagents, Excess Reagents, and Products in Chemical Reactions","strippedTitle":"calculate limiting reagents, excess reagents, and products in chemical reactions","slug":"calculate-limiting-reagents-excess-reagents-and-products-in-chemical-reactions","canonicalUrl":"","seo":{"metaDescription":"Learn to calculate how much product and excess reagent you can expect in a chemical reaction based on your limiting reagent. Given 40.0 grams of ammonia and 50.0 grams of oxygen, what is the limiting reactant? The . It contains well written, well thought and well explained computer science and programming articles, quizzes and practice/competitive programming/company interview Questions. So, the excess reagent is ammonia, and 57.5 g of ammonia will remain when the reaction reaches completion (just subtract 42.5 from 100).

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    Calculate how many grams of nitrogen monoxide and water will be produced if the reaction goes to completion.

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    This problem asks how much of a product is produced. a. write a balance equation for the reaction of nitrogen monoxide with hydrogen to produce nitrogen and water vapor b. write the rate law for this reaction if it is first order in hydrogen and second. Ammonia gas is obtained by the reaction of hydrogen gas and nitrogen gas. Existing hot gas . Nitrogen forms at least three stable oxides: N2O, NO, NO2. The first form of nitrogen produced by the process of mineralization is ammonia, NH 3. Dummies has always stood for taking on complex concepts and making them easy to understand. Nitrogen and hydrogen react to form ammonia, like this: N_2(g) +3H_2(g) rightarrow 2NH_3(g) Use this chemical equation to answer the questions in the table below. All other trademarks and copyrights are the property of their respective owners. a. All numbers following elemental symb, The industrial production of nitric acid is a multistep process. NO 2 dissolves very well in water react with water to give nitrous acid and nitric acid. The balanced chemical equation for this reaction along with all the correct symbols for all the reactant and the products is given below - 4N H3(aq)+3O2(g) 2N 2(g)+6H2O(l) Suggest Corrections 9 Similar questions NH3(g) + 3O2(g) arrow 2N2(g) + 6H2O(g), Nitrogen and hydrogen react to form ammonia according to the following balanced equation: N_2(g) + 3H_2(g) to 2NH_3(g). What is the maximum mass of Ammonia and oxygen react to form nitrogen. When 92.50 moles hydrogen reacts, what quantity (moles) of nitrogen is consumed and what quantity (moles) of ammonia is produced? How much nitrogen was formed? Ammonia gas is formed from nitrogen gas and hydrogen gas, according to the following equation: N2 (g) + 3H2 (g) = 2NH3 (g) If 84.0 g of nitrogen gas is allowed to react with an excess of hydrogen gas to produce 85.0 g of ammonia, what is the percent yiel. c. If 24 grams of water are produced, how many moles of nitrogen monoxide are formed? Calculate the moles of ammonia needed to produce 1.70 mol of nitrogen monoxide. Calculate the moles of ammonia needed to produce 2.10 mol of nitrogen monoxide. How many liters of ammonia gas can be formed from 23.7 L of hydrogen gas at 93.0 degrees C and a pressure of 38.9 kPa? Calculate the number of moles of nitrogen monoxide needed for 2.5 moles of oxygen to react. How many liters of ammonia gas can be formed from 13.7 L of hydrogen gas at 93.0^o C and a pressure of 2.25 atm? The following equation shows how nitrogen dioxide reacts with water to produce nitric acid: 3NO_2(g) + H_2O(l) \to 2HNO_3(l) + NO(g) Predict the sign of \Delta S^\circ for this reaction. How many liter of NO are produced when 2.0 liters of oxygen reacts with ammonia? Ammonia and oxygen react to form nitrogen monoxide gas and water vapour. Balance the above equation. If 7.35 L of nitrogen gas and 26.04 L of hydrogen gas were allowed to react, how many liters of ammonia gas could form? Give the balanced equation for this reaction. 2 See answers Advertisement Myotis 4NH3 + 5O2 ------> 4NO + 6H2O How many moles of ammonia will react with 6.73g of oxygen? Using the above equation, at STP, when 0.675 L of ammonia burns, what volume of water vapor will be formed? The one you have in excess is the excess reagent. Given the equation N2(g) + 3H2(g) = 2NH3(g) determine how many moles of H2 are needed to react with 1.0 mol of N2? You'll run out of oxygen before you run out of ammonia, so oxygen is the limiting reagent. Urea is used as a fertilizer because it can react with water to release ammonia, which provides nitrogen to plants. When 36.3 L of ammonia and 39.0 L of oxygen gas at STP burn, nitrogen monoxide and water are produced. Write a balanced equation for this reaction. 11) Un-thinkable (I'm Ready G gaseous water formula - GOL V Carbonic acid can form water and carbon dioxide upon heating. When 4 litres of nitrogen gas react with 6 litres of hydrogen gas at constant temperature and pressure, how many litres of ammonia gas will be produced? ","hasArticle":false,"_links":{"self":"https://dummies-api.dummies.com/v2/authors/9160"}},{"authorId":34803,"name":"Peter J. Mikulecky","slug":"peter-j-mikulecky","description":"

    Christopher Hren is a high school chemistry teacher and former track and football coach. An explosive whose chemical formula is C_3H_6N_6O_6 produces water, carbon dioxide, and nitrogen gas when detonated in oxygen. What is the balanced chemical equation for this reaction? Ex. Ammonia (NH_3) reacts with oxygen (O_2) to produce nitrogen monoxide (NO) and water (H_2O). What is the limiting reactant? So, the excess reagent is ammonia, and 57.5 g of ammonia will remain when the reaction reaches completion (just subtract 42.5 from 100). Write the balanced equation for this reaction. a. `One way to make ammonia is to synthesize it directly from elemental nitrogen and hydrogen (though this isn't that easy). How many grams of NH_3 can be produced from 2.66 mol of N_2 and ex. Solution Ammonia ( N H3) reacts with oxygen ( O2) to form nitrogen ( N 2) and water ( H2O ). Ammonia is produced by synthesizing nitrogen and hydrogen gas, if i have 2 moles of nitrogen gas and 5 moles of hydrogen gas. The equation for this reaction would be N2 + 3 H2 ---> 2 NH3. A sample of NH_3 gas is completely decomposed to nitrogen and hydrogen gases. Our experts can answer your tough homework and study questions. It also can be interpreted as: 4 molesof NH3reacts with 5 molesof O 2to produce 4 molesof NO and 6 molesof NO 2 is an intermediate in the industrial synthesis of nitric acid, millions of tons of which are produced each year for use primarily in the production of fertilizers.At higher temperatures it is a reddish-brown gas. Write the balanced equation for this reaction. Nitrogen monoxide can be formed according to the equation: N2(g) + 2O2(g) -> 2NO2(g) If 8.0 L of nitrogen is reacted at STP (this is important), exactly how many liters of oxygen at STP would be needed to allow complete reaction? 2 Calcium hydroxide is more soluble in water than magnesium hydroxide. Nitrogen (N2) in the cylinder of a car reacts with oxygen (O2) to produce the pollutant nitrogen monoxide (NO). Nitrogen, N_2, combines with hydrogen, H_2, to form ammonia, NH_3. 2S (s)+3O2 (g) --> 2SO3 (g) 1.09 1024 molecules oxygen Reacting 3.00 mol nitrogen gas with 3.59 mol hydrogen gas will produce how many moles of ammonia according to the following balanced chemical equation? What mass of water is produced by the reaction of 1.09 g of oxygen gas? Assume complete reaction to products. Ammonia is produced by the reaction of hydrogen and nitrogen. Don't waste time or good thought on an unbalanced equation. Ammonia gas decomposes according to the following equation: 2 N H 3 N 2 + 3 H 2 . (c) Give the amount of the excess reac, Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3NO2(g)+H2O(l)?2HNO3(l)+NO(g) Suppose that 4.0 mol NO2 and 0.50 mol H2O combine and react comp. Nitrogen dioxide is an acidic gas. Ammonia burns in oxygen according to the following equation: 4NH_3 + 3O_2 \rightarrow 2N_2 + 6H_2O How many moles of nitrogen gas are generated by the complete reaction of 6.65 moles of ammonia? You can do it by combusting ammonia. (29 mole) b. How many liters of ammonia at STP are produced when 10 g of hydrogen is combined with nitrogen? The balanced form of the given equation is

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    Two candidates, NH3 and O2, vie for the status of limiting reagent. Ammonia and oxygen react to form nitrogen monoxide and water. A. Besides, specific value-added products can be produced by an appropriate . The . How many liters of ammonia are produced when 10.0 g of hydrogen is combined with nitrogen? Calculate ?S in J/K for the reaction of ammonia vapor with fluorine gas to form nitrogen trifluoride gas and hydrogen fluoride gas. When nitrogen gas reacts with chlorine gas, the product is gaseous dinitrogen trichloride. ","hasArticle":false,"_links":{"self":"https://dummies-api.dummies.com/v2/authors/9161"}},{"authorId":9160,"name":"Chris Hren","slug":"chris-hren","description":"

    Christopher Hren is a high school chemistry teacher and former track and football coach. Identify the excess reagent, as well as how many grams of the excess reagent will remain when the reaction reaches completion. To determine the grams of nitrogen monoxide that are generated by the complete reaction of oxygen, start with the assumption that all 100 g of the oxygen react: So, 75 g of nitrogen monoxide will be produced. Image transcription text All other trademarks and copyrights are the property of their respective owners. Given the balanced chemical equation. For the reaction represented by the equation N_2 + 3H_2 to 2NH_3, how many moles of nitrogen are required to produce 18 mol of ammonia? Use trhe balanced equation to change moles of NH3 to moles of NO. N29g)+3H2 (g) --> 2nh3 (g) Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation 3NO_2(g) + H_2O(l) ? For this calculation, you must begin with the limiting reactant. When 36.3 L of ammonia and 39.0 L of oxygen gas at STP burn, nitrogen monoxide and water are produced. Given 40.0 grams of ammonia and 50.0 grams of oxygen, what is the limiting reactant? Reaction of hydrogen and nitrogen to form ammonia Hydrogen gas, H_2, reacts with nitrogen gas, N_2, to form ammonia gas, NH_3, according to the equation 3 H_2 (g) + N_2 (g) to 2NH_3 (g) 1. Ammonia (NH_3) can be formed from nitrogen and hydrogen from the following balanced equation: N_2(g) + 3 H_2(g) \rightarrow 2 NH_3(g) Assuming that all gases are at the same temperature and pressure, calculate how many milliliters of hydrogen gas are ne, When 34.5 L ammonia and 39.5 L oxygen gas at STP burn, nitrogen monoxide and water are produced. What is the total pressure? NH_3 chemically reacts with oxygen gas O_2 to produce nitric oxide NO and water H_2O. Ammonia chemically reacts with oxygen gas to produce nitric oxide and water . In order to find the limiting reagents, excess reagents, and products in this reaction, you need to do the following: Determine the limiting reagent if 100 g of each reagent are present at the beginning of the reaction. Write a balanced chemical equation for Doubtnut 2.59M subscribers Subscribe 3K views 2 years ago Ammonia reacts with oxygen to. NH3 4NH3 + 502 - 4NO + 6H,0 NO H20 O O Question thumb_up 100% Transcribed Image Text: In a closed system, equal amounts of ammonia and oxygen react to produce nitrogen monoxide and water. Nitrogen of ammonia is oxidized to nitrogen gas from -3 oxidation state to 0 oxidation state. 2.33 mol B. Nitrogen, N2, reacts with hydrogen, H2, to form ammonia, NH3. Calculate the moles of oxygen needed to produce \( 0.070 \mathrm{~mol} \) of water. Be sure to write out the . What mass of ammonia is produced when 1.48 L of nitrogen (at STP) react completely in the following equation? Consider the following equation: N_2(g) + 3 H_2(g) ---> 2 NH_3(g) , how many molecules of ammonia are produced when 36.5 litres of hydrogen re STP (in excess nitrogen)? Round your answer to significant digits. Ammonia (N H3) ( N H 3) reacts with oxygen (O2) ( O 2) to produce nitrogen monoxide (NO) and water (H2O) ( H 2 O). You'll run out of oxygen before you run out of ammonia, so oxygen is the limiting reagent.

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    Identify the excess reagent, as well as how many grams of the excess reagent will remain when the reaction reaches completion.

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    To calculate how many grams of ammonia will be left at the end of the reaction, assume that all 100 g of oxygen react:

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    This calculation shows that 42.5 g of the original 100 g of ammonia will react before the limiting reagent is expended. To determine the grams of nitrogen monoxide that are generated by the complete reaction of oxygen, start with the assumption that all 100 g of the oxygen react:

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    So, 75 g of nitrogen monoxide will be produced.

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    Again, assume that all 100 g of the oxygen react in order to determine how many grams of water are produced:

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    You find that 67.5g of water will be produced.

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  • \r\n","description":"In real-life (substances present at the start of a chemical reaction) convert into product.