11. Use the equation below to calculate the following. a. Balance the reaction. 2 KCH;O2 (aq) + H20 (1) + CO2 (g) |K2CO3 (aq) + 2 HC2H3O2 (aq) b. Moles of H2O that can be obtained from 25.0 mL of 0.150 M HC2H3O2 c. Volume of 0.210 M K2CO3 needed to produce 17.5 mol KC2H3O2 d. Volume of 1.25 M HC2H3O2 needed to react with 75.2 mL 0.750 M K2CO3

Chemistry
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Could I have help with B,C,D and I can resubmit the other three. Thank you 

11. Use the equation below to calculate the following.
a. Balance the reaction.
| K2CO3 (aq) + 2 HC2H3O2 (aq) 2 KC2H;O2 (aq) +H2O (1) + CO2 (g)
b. Moles of H2O that can be obtained from 25.0 mL of 0.150 M HC2H3O2
c. Volume of 0.210 M K2CO3 needed to produce 17.5 mol KCH3O2
d. Volume of 1.25 M HC2H302 needed to react with 75.2 mL 0.750 M K2CO3
e. Liters of CO2 gas at 25°C and 0.750 atm, produced by the reaction of 105 mL of 1.50 M HC2H3O2
f. Liters of CO2 gas at 35°C and 0.975 atm, produced by the reaction of 25.0 mL of 0.350M K2CO3 and
25.0 mL of 0.250 M HC2H3O2 (Hint: you need to determine the limiting reactant)
Transcribed Image Text:11. Use the equation below to calculate the following. a. Balance the reaction. | K2CO3 (aq) + 2 HC2H3O2 (aq) 2 KC2H;O2 (aq) +H2O (1) + CO2 (g) b. Moles of H2O that can be obtained from 25.0 mL of 0.150 M HC2H3O2 c. Volume of 0.210 M K2CO3 needed to produce 17.5 mol KCH3O2 d. Volume of 1.25 M HC2H302 needed to react with 75.2 mL 0.750 M K2CO3 e. Liters of CO2 gas at 25°C and 0.750 atm, produced by the reaction of 105 mL of 1.50 M HC2H3O2 f. Liters of CO2 gas at 35°C and 0.975 atm, produced by the reaction of 25.0 mL of 0.350M K2CO3 and 25.0 mL of 0.250 M HC2H3O2 (Hint: you need to determine the limiting reactant)
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