Answer:
The pressure change when a constant volume of gas is heated can be determined using the ideal gas law, which states that PV = nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the ideal gas constant and T is the temperature in kelvins.
Since the volume is constant, we can assume that the change in pressure is proportional to the change in temperature, so we can use the equation:
ΔP = (nRT2 - nRT1) / V
where ΔP is the change in pressure, T2 is the final temperature, and T1 is the initial temperature.
To convert from degrees Celsius to kelvins, add 273.15 to the temperature in degrees Celsius. So, for an initial temperature of 30.0°C, T1 = 30.0 + 273.15 = 303.15 K. And for a final temperature of 40.0°C, T2 = 40.0 + 273.15 = 313.15 K.
Plugging in the values, we have:
ΔP = (nRT2 - nRT1) / V = (n * R * 313.15 - n * R * 303.15) / V = (R * 10) / V = R * 10 / V
The pressure change can be found by multiplying the result by the initial pressure:
ΔP = R * 10 / V * P1 = (8.31 J/mol * K) * 10 / V * 2.00 atm = 16.62 / V atm
The exact pressure change will depend on the volume of the gas, but since the volume is constant, the pressure change will always be equal to 16.62 / V atm.
Step-by-step explanation: