If the temperature of 2.000 moles of an ideal gas is increased by 50$^{\circ}$ C,then what is the increase in the total internal energy?

Question

Quizplus · Accepted Answer

The correct answer is A.The increase in internal energy is given by:$$\Delta U = nC_v\Delta T$$where:* n is the number of moles of gas* $C_v$ is the molar specific heat at constant volume* $\Delta T$ is the change in temperatureFor an ideal gas, $C_v = (3/2)R$, where R is the ideal gas constant.Substituting these values into the equation, we get:$$\Delta U = n(3/2)R\Delta T$$$$\Delta U = (2.000 	ext{ mol})(3/2)(8.314 	ext{ J/mol K})(50 	ext{ K})$$$$\Delta U = 1,247 	ext{ J}$$

If the Temperature of 2 ∘^{\circ}∘ C,then What Is the Increase in the Total Internal Energy

If the Temperature of 2 $^{\circ}$ C,then What Is the Increase in the Total Internal Energy