Question

A 3.50-L fixed-volume flask contains CO(g) at a pressure of 2.00 kPa and a temperature of 25.0 °C. Assuming that carbon monoxide acts as an ideal gas and that its heat capacity is constant over the given temperature range, calculate the change in entropy for the gas when it is heated to 700.0 °C.

Answer 1

To calculate the change in entropy for the gas when heated to 700.0 °C, use the equation ΔS = nCpΔT. Substitute the given values and solve for ΔS.

Step-by-step explanation:

To calculate the change in entropy for the gas when it is heated to 700.0 °C, we can use the equation:

ΔS = nCpΔT

Where, ΔS is the change in entropy, n is the number of moles of gas, Cp is the molar heat capacity at constant pressure, and ΔT is the change in temperature.

In this case, we are assuming carbon monoxide (CO) acts as an ideal gas. The molar heat capacity at constant pressure for an ideal gas is approximately 5/2 R, where R is the gas constant. The change in temperature is 700.0 °C - 25.0 °C. Substitute the values into the equation and solve for ΔS.