5. Using the chemical equation: COg) + 2 H2(g) → CH3OH)a. Starting with 12.5 g H2 and 74.1 g CO, which is limiting reactant?b. What mass of methanol can be obtained (in theory)?c. What mass of the excess reactant is left over?

Answered: Image /qna-images/answer/fcf653f8-50fa-4125-ae28-2fa21825dbe6.jpg

Answered: 5. Using the chemical equation: CO(9) +…

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...

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7. Take the reaction: NH3 + O2 → NO + H2O. In an experiment, 3.25 g of NH3 are allowed to react with 3.50 g of O2. [Hint: Balance the reaction first] a. Which reactant is the limiting reagent? b. How many grams of NO are formed? C. How much of the excess reactant remains after the reaction?
3. If 64.15 g of HCl were produced from 2.07 g of H2 and an excess of Cl2 according to the reaction. A. Write the valid chemical equation.B. What was the percent yield of HCl?
47. For each of the following unbalanced chemical equations, suppose 10.0 g of each reactant is taken. Show by calculation which reactant is the limiting reagent. Calculate the mass of each product that is expected. a. C3HS (g) + O2 (9) → CO2(9) + H20(g) b. Al(s) + Cl2 (g) → AICI3 (s) c. NaOH(s) + C02 (g) → Na2 CO3 (s) + H2O(1) d. NaHCO3 (s) + HCI(aq) → NaCl(aq) + H2 O(1) + CO2 (g)
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A 60.0 g of CaC2 reacts with water to produce C2H2 and 81.2 g of Ca(OH)2. The reaction between these two substances are chemically written as: _______ CaC2 + ______ H2O → _____ C2H2 + _______ Ca(OH)2 Balance the chemical equation. Calculate the molar mass of CaC2 and Ca(OH)2? What is the theoretical yield of Ca(OH)2? What is the percent yield of this reaction if the actual yield of Ca(OH)2 exceeds 2.1 g ?
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1. A mixture of hydrazine (N2H4) and hydrogen peroxide (producing nitrogen and water) is used as a fuel for rocket engines. A. Write the valid chemical equation. B. What mass of N2H4, in grams, is needed to react completely with 35.0 g of H2O2? When, H= 1.01g. O=16.00g. N=14.01g.
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5. Using the chemical equation: CO(9) + 2 H2(g) → CH3OH) a. Starting with 12.5 g H2 and 74.1 g CO, which is limiting reactant? b. What mass of methanol can be obtained (in theory)? c. What mass of the excess reactant is left over?