22. The First Law of Thermodynamics

5.0 g of nitrogen gas at 20°C and an initial pressure of 3.0 atm undergo an isobaric expansion until the volume has tripled.a. What are the gas volume and temperature after the expansion?

5.0 g of nitrogen gas at 20°C and an initial pressure of 3.0 atm undergo an isobaric expansion until the volume has tripled.b. How much heat energy is transferred to the gas to cause this expansion?

5.0 g of nitrogen gas at 20°C and an initial pressure of 3.0 atm undergo an isobaric expansion until the volume has tripled.c. What is the gas pressure after the decrease?

5.0 g of nitrogen gas at 20°C and an initial pressure of 3.0 atm undergo an isobaric expansion until the volume has tripled.d. What amount of heat energy is transferred from the gas as its pressure decreases?

FIGURE CP19.80 shows a thermodynamic process followed by 0.015 mol of hydrogen. How much heat energy is transferred to the gas?

An ideal-gas process is described by p=cV^ /2, where c is a constant.a.Find an expression for the work done on the gas in this process as the volume changes from V₁ to V₂.

n moles of an ideal gas at temperature T1 and volume V1 expand isothermally until the volume has doubled. In terms of n, T₁ , and V₁, what are (a) the final temperature,

n moles of an ideal gas at temperature T1 and volume V1 expand isothermally until the volume has doubled. In terms of n, T₁ , and V₁, what are (b) the work done on the gas, and

n moles of an ideal gas at temperature T1 and volume V1 expand isothermally until the volume has doubled. In terms of n, T₁ , and V₁, what are (c) the heat energy transferred to the gas?

An ideal-gas process is described by p=cV^ /2, where c is a constant.b. 0.033 mol of gas at an initial temperature of 150°C is compressed, using this process, from 300 cm^3 to 200 cm^3. How much work is done on the gas?

n₁ moles of a monatomic gas and n₂ moles of a diatomic gas are mixed together in a container.a. Derive an expression for the molar specific heat at constant volume of the mixture.