Calcium carbonate decomposes upon heating to form calcium oxide and carbon dioxide. A 1.75-g sample of calcium carbonate is placed in an empty, sealed 2.00-L steel container. The container is heated to 625°C and then allowed to cool to 25°C. What is the final pressure (in atm) inside the container? The value of R = 0.0821 L atm mol^-1 K^-1.

Question

Quizplus · Accepted Answer

The correct answer is A because the final pressure inside the container is 0.21 atm. This can be calculated using the ideal gas law, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature. In this case, the number of moles of carbon dioxide produced can be calculated from the mass of calcium carbonate used, and the volume of the container is given. The temperature is converted to Kelvin by adding 273.15 to the Celsius temperature. Plugging these values into the ideal gas law gives the final pressure of 0.21 atm.

Calcium Carbonate Decomposes Upon Heating to Form Calcium Oxide and Carbon