Question

Calcium carbonate, CaCO3(s), the principal compound in limestone, decomposes upon heating to CaO(s) and CO2(g). A sample of CaCO3 is decomposed, and the carbon dioxide is collected in a 250 mL flask. After decomposition is complete, thegas has a pressure of 1.3 atm at a temperature of 31 °C. How many moles of CO2 gas were generated?

Answer 1

Answer:

n = 0.01302 moles

Explanation:

Pressure = 1.3 atm

Temperature = 31 °C + 273 = 304 K ( Converting to kelvin temperature)

Number of moles = ?

Volume = 250 mL = 0.250 L

These quantities are related by the equation below;

PV = nRT

n = PV / RT

n = (1.3 * 0.250) / (0.0821 * 304)

n = 0.01302 moles