A scientist tries to generate a mixture of gases similar to a volcano by introdu

Question

A scientist tries to generate a mixture of gases similar to a volcano by introducing 30.0 g of H2O vapor, 7.5 g of SO2, and 2.0 g of CO2 into a 30.0 L vessel held at 110.0C. (a)Calculate the total pressure of the CO2 in the mixture if the gasses don’t react. However, water and CO2 react to make liquid carbonic acid H2CO3. Write the balanced chemical reaction. Assuming the reaction is complete, how much carbonic acid is formed and how much of each molecule is in the gas phase. Finally, what is the pressure of the mixture if H2CO3 is not in the vapor phase?

Explanation / Answer

m = 30 g of vapor

mol = mass/MW = 30/18 = 1.666666 mol of water

m = 7.5 g of SO2

mol = mass/MW = 7.5/64.066 = 0.117066 mol of SO2

mol of CO2 = mass/MW = 2/44 = 0.0454

total mol = 1.666666+0.117066+0.0454 = 1.829

then

a)

total P

P = nRT/V

P = (1.829)(0.082)(110+273)/(30)= 1.91 atm

b)

reaction for

H2O(g) + CO2(g) = H2CO3(g)

limiting reactant is CO2

0.0454 mol of CO2 = 0.0454 mol of H2CO3

mass = mol*MW = 0.0454*62.03 = 2.82 g of H2CO3

The partial pressure will be similar to CO2

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