Use the equation below to calculate the following. a. Balance the reaction. ___ K2CO3 (aq) + ___ HC2H3O2 (aq) → ___ KC2H3O2 (aq) + ___ H2O (l) + ___ 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 KC2H3O2
Use the equation below to calculate the following. a. Balance the reaction. ___ K2CO3 (aq) + ___ HC2H3O2 (aq) → ___ KC2H3O2 (aq) + ___ H2O (l) + ___ 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 KC2H3O2
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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11. Use the equation below to calculate the following.
a. Balance the reaction. ___ K2CO3 (aq) + ___ HC2H3O2 (aq) → ___ KC2H3O2 (aq) + ___ H2O (l) + ___ 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 KC2H3O2
d. Volume of 1.25 M HC2H3O2 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 0.350 M K2CO3 and 25.0 mL of 0.250 M HC2H3O2 (Hint: you need to determine the limiting reactant)
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