Assuming 1 atm of pressure and room temperature (293.15 K), how many mL of CO2 are produced from one tablet?

Answer 1

Following up the previous question, we use the number of moles of carbon dioxide produced to determine how many mL will be produced. This is done using the Ideal Gas Law:

PV = nRT

Where:

P = pressure in ATM

V = volume in liters

n = number of moles (in our case, 0.0156 per the answer to the previous question)

R = ideal gas constant (0.0821 L *atm * K^-1 * mol^-1)

T = temperature in kelvin

Plugging in our values into the ideal gas law we have:

(1 atm)(V) = (0.0156 mol)(0.0821 L *atm * K^-1 * mol^-1)(293.15K)

Solving for V gives us 0.3755 liters, or 375.5 mL