Hydrogen cyanide gas can be made by a two step process. First, ammonia is reacted with oxygen gas to give nitrogen monoxide and water vapor. In the next step, nitrogen monoxide is reacted with methane (CH4) to give hydrogen cyanide gas. The by-products in the second step are water and hydrogen gas. When 23.9 g of ammonia and 27.4 g of methane are used, how many grams of hydrogen cyanide can be produced? Please do not include units in your answer. Assume both masses have 3 sig figs.

Hydrogen cyanide gas can be made by a two step process. First, ammonia is reacted with oxygen gas to give nitrogen monoxide and water vapor. In the next step, nitrogen monoxide is reacted with methane (CH4) to give hydrogen cyanide gas. The by-products in the second step are water and hydrogen gas. When 23.9 g of ammonia and 27.4 g of methane are used, how many grams of hydrogen cyanide can be produced? Please do not include units in your answer. Assume both masses have 3 sig figs.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Chloroform, CHCl3, reacts with chlorine, Cl2, to form carbon tetrachloride, CCl4, and hydrogen chloride, HCl. In an experiment 25 grams of chloroform and 0.36 mol of chlorine were mixed. Which is the limiting reactant? The equation is given as CHCl3 + Cl2 = CCl4 + HCl
Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s)+3Cl2(g)→2AlCl3(s) You are given 16.0 gg of aluminum and 21.0 gg of chlorine gas. If you had excess aluminum, how many moles of aluminum chloride could be produced from 21.0 gg of chlorine gas, Cl2?
[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant. b) Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 64.7 grams Al according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) c) Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 201 grams Fe₂O₃ according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) d) Which of the following substances is the limiting reactant? e) What is the mass in grams of the excess Fe₂O₃ remaining after the partial reaction of 201 g Fe₂O₃ with 64.7 g Al? Give your answer to three significant figures.
A sample of dry solid waste has the following composition : 531 g carbon (C), 133 g hydrogen (H), and 335 g oxygen(O) . How many liters of air is required to combust the waste.
When propane (C3Hg) reacts with oxygen, carbon dioxide and water are produced. The balanced equation for this reaction is C3 Hs (g) + 502 (g) → 3CO2(g) + 4H2O(g) If 10 moles of oxygen react, The reaction consumes moles of propane (C3H8). The reaction produces moles of carbon dioxide and moles of water.
Liquid octane (CH3(CH2)6CH3) reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. If 64.0g of water is produced from the reaction of 92.52g of octane and 181.4g of oxygen gas, calculate the percent yield of water.
Liquid nitroglycerine (CaHsNaO₂) is a powerful explosive. When it detonates, it produces a gaseous mixture of nitrogen, water, carbon dioxide and oxygen. If 5.55 g of nitroglycerine explodes and 2.98 g of CO₂ is collected, what is the percentage yield of carbon dioxide?
Acid rain is caused in part by burning coal that contains sulfur impurities. The sulfur is converted first to SO2, which reacts with oxygen and atmospheric moisture to produce sulfuric acid, H2SO4. If a particular coal contains 1.90% sulfur (by mass), calculate the mass of sulfuric acid produced by burning a metric ton (1000 kg) of the coal.
Consider the following reaction between sulfur trioxide and water: SO3(g)+H2O(l)→H2SO4(aq) A chemist allows 61.5 g of SO3SO3 and 11.2 g of H2O to react. When the reaction is finished, the chemist collects 56.2 g of H2SO4 Determine the percent yield for the reaction. Express your answer to three significant figures.
The thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid-fuel rockets. In the thermite reaction, iron(III) oxide reacts with elemental aluminum to form aluminum oxide and elemental iron. Write a balanced equation for this reaction. What mass of iron(III) oxide must be used to produce 15.0 g elemental iron? What mass of aluminum oxide will be produced when 15.0 g of iron is produced?
The reaction of carbon and water at a high temperature produces a mixture of hydrogen and carbon monoxide gases. This mixture is known as synthesis gas (or syngas). How many grams of hydrogen gas can be formed from the reaction of 125 g of water with excess carbon?
Consider the chemical equation for the combustion of ammonia: 4NH3(g) + 70,(g) – 4NO,(g) + 6H,0(g) Which statement provides the correct and standard interpretation of the chemical equation? 12 pounds of NH3(g) react with 14 pounds of O,(g) to produce 8 pounds of NO,(g) and 6 pounds of H2O(g). 4 mol of NH3(g) react with 7 O mol of 0,(g) to produce 4 mol of NO,(g) and 6 mol of H,0(g) 89.6 g of NH3(g) react with 156.8 g of O,(g) to produce 89.6 g of NO2(g) and 134.4 g of H2O(g). 22.4 L of NH3(g) react with 22.4 O Lof 0,(g) to produce 22.4 L of NO,(g) and 22.4 L of H2O(g).