Use the References to access important values if needed for this question.According to the following reaction, how many grams of ethylene (C2H4) are required for the complete reaction of 27.9 grams ofhydrogen gas?Masshydrogen (g) + ethylene (C2H4)(g) →ethane (C2H6) (g)grams ethylene (C2H4)

388.2 Explanation:The balanced chemical equation for the reaction is:H2(g)+C2H4(g)→C2H6(g) From…

Answered: Use the References to access important…

World of Chemistry

7th Edition

ISBN:9780618562763

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 55A

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For the chemical reaction C3H8O2+4O23CO2+4H2O how many product molecules are formed when nine C3H8O2 molecules react?
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?
4.72 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.
4.70 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. (c) identify the limiting reactant, and explain how the pictures allow you to do so.
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.
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.
4.71 The particulate scale drawing shown depict the products of a reaction between N2 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. (c) Identify the limiting reactant, and explain how the pictures allow you to do so.
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.
Calculate the amounts of reactants needed in a chemical reaction to produce a specified amount of product.
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
list at least three quantities that must be conserved in chemical reactions.
3.75 The following pictures show a molecular-scale view of a chemical reaction between the compounds AB2 and B2. (A atoms are shown in blue and B atoms in white). 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 reac- tion has gone to completion. Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.

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Use the References to access important values if needed for this question. According to the following reaction, how many grams of ethylene (C2H4) are required for the complete reaction of 27.9 grams of hydrogen gas? Mass hydrogen (g) + ethylene (C2H4)(g) →ethane (C2H6) (g) grams ethylene (C2H4)