An ideal gas is heated at a constant pressure of 1.80 × 105 Pa from a temperature of -73.0°C to a temperature of +27.0°C. The initial volume of the gas is 0.100 m³. The heat energy supplied to the gas in this process is 40.0 kJ. What is the increase in internal energy of the gas? -8.95:kJ

An ideal gas is held at a constant temperature of 370 K as it expands slowly from a volume of 0.70 m³ to 6.0 m³. As the gas expands, it does 120 J of work. What is the change in the internal energy AU of the gas during this process? AU = J How much heat Q is absorbed by the gas as it expands? Q = J

Work Done by a Gas: A gas expands from an initial volume of 0.040 m3 and an initial pressure of 210 kPa to a final volume of 0.065 m3 while its temperature is kept constant. How much work is done by the gas? (R = 8.31 J/mol ∙ K) Work Done by a Gas: A gas expands from an initial volume of 0.040 m3 and an initial pressure of 210 kPa to a final volume of 0.065 m3 while its temperature is kept constant. How much work is done by the gas? (R = 8.31 J/mol ∙ K)

2.40 moles of nitrogen gas at 252 K are kept in a container. (a) If the temperature of the gas is increased to 500 K at constant volume, how much heat was transferred to the gas? The molar specific heat capacity of nitrogen at constant volume is 20.8 J/mol. ­­­­­_________J (b) What is the change in internal energy of the gas due to this change in temperature at constant volume? _________J (c) Suppose the temperature of the gas is increased from 252 K to 500 K at constant pressure, how much heat is transferred to the gas? The molar specific heat capacity of nitrogen at constant pressure is 29.1 J/mol. _________J (d) How much work is done on the gas as its temperature increases at constant pressure? _________J