Question

1.The pressure of a gas remains constant while the temperature, volume, and internal energy of the gas increase by 52.7 Co, 1.48 x 10-3 m3, and 946 J, respectively. The mass of the gas is 29.9 g, and its specific heat capacity (at constant pressure) is 1060 J/(kg Co). Determine the pressure. 2. Under constant-volume conditions, 3600 J of heat is added to 1.9 moles of an ideal gas. As a result, the temperature of the gas increases by 65.1 K. How much heat would be required to cause the same temperature change under constant-pressure conditions? Do not assume anything about whether the gas is monatomic, diatomic, etc.

Answer 1

While a gas's temperature, volume, and internal energy rise, its pressure stays constant. An ideal gas sample is heated while maintaining a fixed pressure.

The temperature of a cylinder containing an ideal gas with fixed mass and constant volume is changed. At constant pressure of 2.0 atm, the volume of an ideal gas is dropped from 5.0 L to 5.0 mL. Calculate the work required for this process in J. Assuming the environment is always at a constant 300:0 K temperature and pressure, Without adding or removing heat, the volume of a perfect monoatomic gas is squeezed to halve.

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