The drawing below shows a mixture of molecules: key carbon hydrogen nitrogen sulfur охудen chlorine Suppose the following chemical reaction can take place in this mixture: CO(g)+2 H,(g) → CH,OH(g) Of which reactant are there the most initial moles? Enter its chemical formula: Of which reactant are there the least initial moles? Enter its chemical formula: Which reactant is the limiting reactant? Enter its chemical formula:

The drawing below shows a mixture of molecules: key carbon hydrogen nitrogen sulfur охудen chlorine Suppose the following chemical reaction can take place in this mixture: CO(g)+2 H,(g) → CH,OH(g) Of which reactant are there the most initial moles? Enter its chemical formula: Of which reactant are there the least initial moles? Enter its chemical formula: Which reactant is the limiting reactant? Enter its chemical formula:

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 44QAP: Balance the following chemical equation, and then answer the question below....

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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.
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.
Propane, C3H8, is the fuel of choice in a gas barbecue. When burning, the balanced equation is C3H8+5O23CO2+4H2O a What is the limiting reactant in cooking with a gas grill? b If the grill will not light and you know that you have an ample flow of propane to the burner, what is the limiting reactant? c When using a gas grill you can sometimes turn the gas up to the point at which the flame becomes yellow and smokey. In terms of the chemical reaction, what is happening?
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.
4.8 In an experiment carried out at very low pressure, 13x1015 molecules of H2 are reacted with acetylene, C2H2, to form ethane, C2H6, on the surface of a catalyst. Write a balanced chemical equation for this reaction. How many molecules of acetylene are consumed?
4.37 The theoretical yield and the actual yield for various reactions are given below. Determine the corresponding percentage yields. Theoretical Yield Actual Yield Reaction 1 35.0 g 12.8 g Reaction 2 9.3 g 120 mg Reaction 3 3.7 metric tons 1250 kg Reaction 4 40.0 g 41.0 g
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).
3.50 A test of an automobile engine's exhaust revealed that g of NO2 was emitted in 10 minutes of operation. How many moles of NO2 would this engine release if it were used for a 45-minute commute, assuming that this mea- sured number is representative of the emission under all circumstances?
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.
Consider the unbalanced equation for the combustion of propane: :math>C3H8(g)+O2(g)CO2(g)+H2O(g) rst, balance the equation. Then, for a given amount of propane, write the mole ratios that would enable you to calculate the number of moles of each product as well as the number of moles of O2that would be involved in a complete reaction. Finally, show how these mole ratios would be applied if 0.55 mole of propane is combusted.
4.69 The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH. The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.