A container is filled with an ideal diatomic gas to a pressure and volume of P₁ and V₁, respectively. The gas is then warmed in a two-step process that increases the pressure by a factor of four and the volume by a factor of five. Determine the amount of energy transferred to the gas by heat if the first step is carried out at constant volume and the second step at constant pressure. (Use any variable or symbol stated above as necessary.) Q = 63.5 The gas is in three different states. See if you can determine the pressure, volume, and temperature for each state and then the change in temperature during the two processes. Find expressions for the amount of heat supplied during isovolumetric and isobaric processes. Knowing the amounts of heat supplied during each process, how can you determine the total amount of heat supplied?

When air expands adiabatically (without gaining or losing heat), its pressure P and volume V are related by the equation PV to the power of 1.4 = C where C is a constant. Suppose that at a certain instant the volume is 480 cubic centimeters and the pressure is 75 kPa and is decreasing at a rate of 10 kPa/minute. At what rate in cubic centimeters per minute is the volume increasing at this instant? Please Write legible

1 kg of air is reversibly heated at constant pressure from an initial state of 300 K and 1 bar until its volume increases to three times its initial value. Determine the internal energy changes, entapy, and heat and work requirements for this process. The molar mass of air is 28.9 g / mol. Write down all your assumptions made. w= dU= dH= Q=

A container is filled with an ideal diatomic gas to a pressure and volume of P1 and V1, respectively. The gas is then warmed in a two-step process that increases the pressure by a factor of five and the volume by a factor of four. Determine the amount of energy transferred to the gas by heat if the first step is carried out at constant volume and the second step at constant pressure. (Use any variable or symbol stated above as necessary.)

A cylinder contains 0.250 mol of carbon dioxide (CO₂) gas at a temperature of 27.0°C. The cylinder is provided with a frictionless piston, which maintains a constant pressure of 1.00 atm on the gas. The gas is heated until its temperature increases to 127.0°C. Assume that the CO₂ may be treated as an ideal gas. Express your answer in joules. AU = Submit Part D Submit How much heat was supplied to the gas? Express your answer in joules. Part E W₁ = ΑΣΦ | Submit Request Answer ΑΣΦ Request Answer Request Answer < Return to Assignment Provide Feedback www How much work would have been done if the pressure had been 0.50 atm? Express your answer in joules. VE ΑΣΦ P Pearson = ? ? J ? J J

Part A: If you supply 2950 J of heat to 6.00 moles of an ideal diatomic gas initially at 23.0 ∘C in a perfectly rigid container, what will be the final temperature of the gas? Express in degrees Celsius. Part B: Suppose the gas in the container were an ideal monatomic gas instead. How much heat would you need to add to produce the same temperature change? Part C: Which pV diagram expresses these processes?