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For the following unbalanced chemical equation, suppose that exactly 1.40 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of CO2 is expected (assuming that the limiting reactant is completely consumed). CS: (1) + O2(9) → CO2(9) + SO2(9) Limiting reactant: Mass of CO2 = For the following unbalanced chemical equation, suppose that exactly 1.95 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of H2O is expected (assuming that the limiting reactant is completely consumed). NH3 (9) + CO2(9) → CN;H,O(s) + H2O(1) Limiting reactant: Mass of H20 = For the following unbalanced chemical equation, suppose that exactly 1.95 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of H2O is expected (assuming that the limiting reactant is completely consumed). H2(9) + MnO2(s) → MnO(s) + H2O(1) Limiting reactant: Mass of H20 =| For each of the following unbalanced chemical equations, suppose that exactly 1.65 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of ICI is expected (assuming that the limiting reactant is completely consumed L(s) + Cl2(9) → ICI(9) Limiting reactant: Mace of ICL -

For the following unbalanced chemical equation, suppose that exactly 1.40 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of CO2 is expected (assuming that the limiting reactant is completely consumed). CS: (1) + O2(9) → CO2(9) + SO2(9) Limiting reactant: Mass of CO2 = For the following unbalanced chemical equation, suppose that exactly 1.95 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of H2O is expected (assuming that the limiting reactant is completely consumed). NH3 (9) + CO2(9) → CN;H,O(s) + H2O(1) Limiting reactant: Mass of H20 = For the following unbalanced chemical equation, suppose that exactly 1.95 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of H2O is expected (assuming that the limiting reactant is completely consumed). H2(9) + MnO2(s) → MnO(s) + H2O(1) Limiting reactant: Mass of H20 =| For each of the following unbalanced chemical equations, suppose that exactly 1.65 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of ICI is expected (assuming that the limiting reactant is completely consumed L(s) + Cl2(9) → ICI(9) Limiting reactant: Mace of ICL -

Chemistry
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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a For the following unbalanced chemical equation, suppose that exactly 1.40 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of CO2 is expected (assuming that the limiting reactant is completely consumed). CS2 (1) + O2 (9) → CO2(g) + SO2(9) Limiting reactant: Mass of CO2 g b For the following unbalanced chemical equation, suppose that exactly 1.95 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of H2O is expected (assuming that the limiting reactant is completely consumed). NH3 (9) + CO2 (g) → CN2H40(s) + H,O(1) Limiting reactant: Mass of H2 O = g C For the following unbalanced chemical equation, suppose that exactly 1.95 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of H2O is expected (assuming that the limiting reactant is completely consumed). H2 (g) + MnO2(s) → MnO(s) +H2O(1) Limiting reactant: Mass of H2 0 = g d For each of the following unbalanced chemical equations, suppose that exactly 1.65 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of ICl is expected (assuming that the limiting reactant is completely consumed). I2 (s) + Cl2 (9) → ICI(g) Limiting reactant: Mass of ICl = |g
Transcribed Image Text:a For the following unbalanced chemical equation, suppose that exactly 1.40 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of CO2 is expected (assuming that the limiting reactant is completely consumed). CS2 (1) + O2 (9) → CO2(g) + SO2(9) Limiting reactant: Mass of CO2 g b For the following unbalanced chemical equation, suppose that exactly 1.95 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of H2O is expected (assuming that the limiting reactant is completely consumed). NH3 (9) + CO2 (g) → CN2H40(s) + H,O(1) Limiting reactant: Mass of H2 O = g C For the following unbalanced chemical equation, suppose that exactly 1.95 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of H2O is expected (assuming that the limiting reactant is completely consumed). H2 (g) + MnO2(s) → MnO(s) +H2O(1) Limiting reactant: Mass of H2 0 = g d For each of the following unbalanced chemical equations, suppose that exactly 1.65 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of ICl is expected (assuming that the limiting reactant is completely consumed). I2 (s) + Cl2 (9) → ICI(g) Limiting reactant: Mass of ICl = |g
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