In a sealed vessel at 25 C and 689 mmHg, 150 mL of a 1.33M acetic acid solution is added to 225 mL of a 0.899 M sodium carbonate solution. ?
The reaction proceeds according to the reaction below—-
2HC2H3O2 + Na2CO3 >>>>> 2NaC2H3O2 + H2O +CO2
How many moles of CO2 can be produced by the acetic acid solution?
How many moles of CO2 can be produced by the Sodium Carbonate solution?
Based on the limiting reagent, how many moles of CO2 are actually produced?
Based on the number of moles of CO2 produced, how many liters of gas are collected if the gas is collected at a temperature of 25C and a pressure of 689 mmHg?
Please list the steps. I am very lost and confused.
- hcbiochemLv 74 weeks ago
Moles HC2H3O2 = 0.150 L X 1.33 mol/L = 0.1995 mol
0.1995 mol HC2H3O2 X (1 mol CO2 / 2 mol HC2H3O2) = 0.09975 mol CO2
Moles Na2CO3 = 0.225 L X 0.899 mol/L = 0.202 mol
0.2023 mol Na2CO3 X (1 mol CO2 / 1 mol Na2CO3) = 0.2023 mol CO2
Acetic acid is the limiting reactant because the amount available will allow the production of only 0.0998 moles of CO2
Calculate the volume using the ideal gas law:
PV = n RT
(689 / 760) V = 0.0998 mol (0.08206 Latm/molK) (298 K)
V = 2.69 L CO2