CH4(g) + 2 Cl2(g) → CH2C12(g) + 2 HCI(g) CH4 reacts with Cl2 as shown by the equation above. A chemist adds 1.35 moles of CH4 is placed in a reaction vessel containing 3.58 mol of Cl2(g). (a) Identify the limiting reactant. Justify your answer with a calculation. (b) Calculate the total number of moles of CH2CI2(g) in the container after the limiting reactant has been totally consumed. (c) Calculate the total moles of the excess reactant left over. (d) If 0.95 moles of CH,Cl, are produced in the lab, what is the percent yield?

CH4(g) + 2 Cl2(g) → CH2C12(g) + 2 HCI(g) CH4 reacts with Cl2 as shown by the equation above. A chemist adds 1.35 moles of CH4 is placed in a reaction vessel containing 3.58 mol of Cl2(g). (a) Identify the limiting reactant. Justify your answer with a calculation. (b) Calculate the total number of moles of CH2CI2(g) in the container after the limiting reactant has been totally consumed. (c) Calculate the total moles of the excess reactant left over. (d) If 0.95 moles of CH,Cl, are produced in the lab, what is the percent yield?

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

A sample of 1.527moles of methane (CH4) is mixed with 1.32 moles of chlorine. What is the theoretical yield, in moles, of CCl4 that can be made from these amounts? CH₁ (g) +4 Cl2 (g) → CCl4 (1) + 4 HCl (g)
Methanol (CH 4O), which is used as a fuel in highperformance racing cars, burns in the presence of O 2 to form CO 2 and H 2O. The molar masses for all substances are given under the balanced equation. 2 CH4O(l) + 3 O2(g)----------> 2 CO2(g) + 4 H2O(g) 32.04 g/mol 32.00 g/mol 44.01 g/mol 18.02 g/mol a. What is the theoretical yield of CO 2 from 48.0 g of methanol? b. What is the percent yield of CO 2 if 48.0 g of CO 2 are formed?
what mass of calcium hydroxide in grams is needed to produce 5.11 mol of water?
Consider the following equation: 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (l) When 6.97 moles of ammonia (NH3) react with excess oxygen, calculate the total number of moles of products. You do not need to include units with your answer. Notice that this question is a bit different. You are asked for the sum of both products.
The following are actual student responses to the question: “Why is it necessary to balance chemical equations?” (a) The chemicals will not react until you have added the correct mole ratios. (b) The correct products will not be formed unless the right amount of reactants have been added. (c) The balanced equation tells you how much reactant you need and allows you to predict how much product you’ll make. (d) A mole-to-mole ratio must be established for the reaction to occur as written. Which statement is the correct or best response? Justify your choice. Why do you think the other statements are incorrect? Explain. Which statement is the correct or best response? Justify your choice. Why do you think the other statements are incorrect? Explain.
A 18.2 g of iron metal reacts with excess oxygen gas to produce 47.9 g of Fe3O4. The reaction between these two substances are written as: ____ Fe(s) + ____ O2(g) → _____ Fe3O4 (s) Balance the chemical equation. Calculate the molar mass of O2 and Fe3O4. If the 43.72 g of Fe3O4 was produced, what is the percent yield of this reaction?
The Haber process is used to industrially produce ammonia ( NH3 ) . Ammonia is the active ingredient in a variety of household cleaners . The data table below summarizes the experimental quantities of reactants and products collected from a specific batch. If the company chemist calculated that 12,163 g of NH3 should be produced, what is the percent yield
This question has two parts and requires two answers. Consider the reaction 4 Fe + 3 02→ 2 Fe203 a) What is the theoretical yield, in grams, of iron(III) oxide if 20.0 g of iron are mixed with 10.5 grams of oxygen gas? b) What is the limiting reactant?
The theoretical yield of reactions Consider the reaction 1CO(g) + O2 (g) --> 2CO2(g) if 9.420 g CO is mixed with 16.84g O2, CALCULATE THE THEORETICAL YIELD (g) of CO2 produced by the reaction.
A reinforced steel cylinder is filled with 21.0 moles of hydrogen and 12.0 moles of oxygen. The mixture is detonated inside the cylinder causing the following reaction to take place. 2 H2(g) + O2(g) → 2 H2O (g) What is the theoretical yield, in grams, of the reaction?
The limiting reactant is the reactant that is completely consumed in chemical reactions and determines the theoretical yield of reactions. When solid iron filings are added to a solution of copper(II) sulfate, an redox reaction occurs to form copper metal and one of two possible iron sulfate compounds. The unbalanced equations for the two possible reactions are given below. If 1.152 g of the Fe (the limiting reactant) are used, what is the theoretical yield according the balanced equation for reaction 1? Reaction 1: CuSO4(aq) + Fe(s) ⟶ ⟶ FeSO4(aq) + Cu(s) Reaction 2: CuSO4(aq) + Fe(s) ⟶ ⟶ Fe2(SO4)3(aq) + Cu(s)
The poisonous gas hydrogen cyanide (HCN) is producedby the high-temperature reaction of ammonia with methane (CH4). Hydrogen is also produced in this reaction.(a) Write a balanced chemical equation for the reactionthat occurs.(b) Suppose 500.0 g methane is mixed with 200.0 g ammonia. Calculate the masses of the substances present afterthe reaction is allowed to proceed to completion.