QUESTION 10 Which of the following statements about the limiting reactant is true? O After the reaction is complete, there will be some amount of the fimiting reactant in your container along with the products. O The amount of the limiting reactant determines the amount of all the products you obtain in a chemical reaction. O The limiting reactant is found on the right-hand side of a chemical equation. O The amount of the limiting reactant increases during a chemical reaction until it is equal with the amount of the excess reactant.

QUESTION 10 Which of the following statements about the limiting reactant is true? O After the reaction is complete, there will be some amount of the fimiting reactant in your container along with the products. O The amount of the limiting reactant determines the amount of all the products you obtain in a chemical reaction. O The limiting reactant is found on the right-hand side of a chemical equation. O The amount of the limiting reactant increases during a chemical reaction until it is equal with the amount of the excess reactant.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 42QAP: Explain how one determines which reactant in a process is the limiting reactant. Does this depend...

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Balance the following chemical equation, and then answer the question below. :math>CuSO4(aq)+KI(s)CuI(s)+I2(s)+K2SO4(aq) ich reactant is the limiting reactant? Choose the best answer. th CuSO4and Kl are equally limiting because they react in a 1:1 mole ratio. i>CuSO4is the limiting reactant because only 2 moles are available compared with 4 moles of Kl. i>Kl is the limiting reactant because it is present in excess. i>Neither CuSO4 nor Kl is a limiting reactant because 6 total moles are present on the reactant side compared with 5 total moles on the product side. i>The limiting reactant cannot be determined because the starting amounts are not given.
Classify each of the following statements as true or false: a Coefficients in a chemical equation express the molar proportions among both reactants and products. b A stoichiometry problem can be solved with an unbalanced equation. c In solving a stoichiometry problem, the change from quantity of given substance to quantity of wanted substance is based on masses. d Percentage yield is actual yield expressed as a percentage of ideal yield. e The quantity of product of any reaction can be calculated only through the moles of the limiting reactant. f rH is positive for an endothermic reaction and negative for an exothermic reaction.
4.72 The picture shown depicts the species present at the start of a combustion reaction between methane, CH4 and oxygen, O2 (a) What is the limiting reactant? (b) Draw the resulting state after this set of reactants has reacted as far as possible.
Explain how one determines which reactant in a process is the limiting reactant. Does this depend only on the masses of the reactant present? Give an example of how to determine the limiting reactant by using a Before-Change-After (RCA) table with a balanced chemical equation and reactant starling amounts.
Alkali metal hydroxides are sometimes used to “scrub” excess carbon dioxide from the air in closed spaces (such as submarines and spacecraft). For example, lithium hydroxide reacts with carbon dioxide according to the unbalanced chemical equation :math>LiOH(s)+CO2(g)Li2CO3(s)+H2O(g) ppose a lithium hydroxide canister contains 155 g of LiOH(s). What mass of CO2(g)will the canister be able to absorb? If it is found that after 24 hours of use the canister has absorbed 102 g of carbon dioxide, what percentage of its capacity has been reached?
Ammonia can be formed by a direct reaction of nitrogen and hydrogen. N2(g) + 3 H2(g) 2 NH3(g) A tiny portion of the starting mixture is represented by the diagram, where the blue circles represent N and the white circles represent H. Which of these represents the product mixture? For the reaction of the given sample, which of these statements is true? (a) N2 is the limiting reactant. (b) H2 is the limiting reactant. (c) NH, is the limiting reactant. (d) No reactant is limiting: they are present in the correct stoichiometric ratio.
In a blast furnace at high temperature, iron(III) oxide in ore reacts with carbon monoxide to produce metallic iron and carbon dioxide. The liquid iron produced is cooled and weighed. The reaction is run repeatedly with the same initial mass of iron(III) oxide, 19.0 g, but differing initial masses of carbon monoxide. The masses of iron obtained arc shown in this graph. (a) Write the balanced chemical equation for this reaction. (b) Calculate the mass of CO required to react completely with 19.0 g iron(III) oxide. (c) Calculate the mass of carbon dioxide produced when the reaction converts 10.0 g iron(III) oxide completely to products. (d) From the graph, determine which reactant is limiting when less than 10.0 g carbon monoxide is available to react with 19.0 g iron(III) oxide. (e) From the graph, determine which reactant is limiting when more than 10.0 g carbon monoxide is available to react with 19.0 g iron(III) oxide. (f) Calculate the percent yield if 24.0 g iron(III) oxide reacted with 20.0 g carbon monoxide to produce 15.9 g metallic iron. (g) Calculate the minimum mass of additional limiting reactant required to react with all of the excess of nonlimiting reactant from part (f).
3.81 The particulate scale drawing shown depicts the products of a reaction between H2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients.
Small quantities of ammonia gas can be generated in the laboratory by heating an ammonium salt with a strong base. For example, ammonium chloride reacts with sodium hydroxide according to the following balanced equation: :math>NH4Cl(s)+NaOH(s)NH3(g)+NaCl(s)+N2O(g) at mass of ammonia gas is produced if 1.39 g of ammonium chloride reacts completely?
Consider the equation: 2A+B5C. If 10.0 g of A reacts with 5.00 g of B. how is the limiting reactant determined? Choose the best answer and explain. l type='a'> Choose the reactant with the smallest coefficient in the balanced chemical equation. So in this case, the limiting reactant is B. Choose the reactant with the smallest mass given. So in this case, the limiting reactant is The mass of each reactant must be converted to moles and then compared to the ratios in the balanced chemical equation. So in this case, the limiting reactant cannot be determined without the molar masses of A and B. The mass of each reactant must he converted to moles first. The reactant with the fewest moles present is the limiting reactant. So in this case, the limiting reactant cannot be determined without the molar masses of A and B. The mass of each reactant must be divided by their coefficients in the balanced chemical equation, and the smallest number present is the limiting reactant. So in this case, there is no limiting reactant because A and B arc used up perfectly.
You have seven closed containers, each with equal masses of chlorine gas (Cl2) . You add 10.0 g of sodium to the first sample, 20.0 g of sodium to the second sample, and so on (adding 70.0 g of sodium to the seventh sample). Sodium and chlorine react to form sodium chloride according to the equation 2Na(s)+Cl22NaCl(s) After each reaction is complete, you collect and measure the amount of sodium chloride formed. A graph of your results is shown below. Answer the following questions: a. Explain the shape of the graph. b. Calculate the mass of NaCl formed when 20.0 g of sodium is used. c. Calculate the mass of Cl2 in each container. d. Calculate the mass of NaCl formed when 50.0 g of sodium is used. e. Identify the leftover reactant, and determine its mass for parts b and d above.
Consider the following balanced chemical equation: A+5B3C+4D a. Equal masses of A and B are reacted. Complete each of the following with either A is the limiting reactant because ; B is the limiting reactant because ____ ; or we cannot determine the limiting reactant because _____ i. If the molar mass of A is greater than the molar mass of B, then ii. If the molar mass of B is greater than the molar mass of A, then b. The products of the reaction are carbon dioxide (C) and water (D). Compound A has a similar molar mass to carbon dioxide. Compound B is a diatomic molecule. Identify compound B, and support your answer. c. Compound A is a hydrocarbon that is 81.7 1% carbon by mass. Determine its empirical and molecular formulas.