The figure shows two pathways for a sample of an ideal diatomic gas which is expanding in volume in going from A to C where path AC is an isothermal process. (Assume f= 5 for this diatomic gas.) P/103 Pa 4.00 A 3.50 3.00 2.00 1.59 B 1.00 0 2.50 0.00 1.00 2.00 5.50 3.00 4.00 5.00 6.00 V/m³ Drag/drop the following equations/values into the boxes below and hence determine the quantities required (note that you can only drop an item into a box with a matching colour). Please state all values in scientific notation and to the appropriate number of significant figures. Note that the following relationships are for an ideal gas with an initial state (P1, V1, T₁) and a final state (P2, V2, T2) where W is the work done on the gas, Q is the heat transferred to the gas and AU is the change in internal energy of the gas. Cp and Cy are the heat capacities of the gas at constant pressure and constant volume respectively. Q=0 Q= CPAT Q = CVAT Q=-w Q = nRT In (V2/V1) W=0 W=-Q W=-PAV W=-nRT In (V2/V1) W= (P2V2-P1V1) AU=0 AU = W AU=Q+W PV = nRT (i) Complete the table below for path AC (an isothermal process). Drag and drop items into the first row and then calculate the values and enter the numbers in the second row. change in internal energy heat transferred to the gas work done on the gas J J

Question 1. An ideal diatomic gas contracts from 1.25 m³ to 0.500 m³ at a constant pressure of 1.50 x 10°P.. Draw a PV diagram and name this process that occurs at constant pressure. If the initial temperature is 425 K, calculate (a) the work done on the gas, (b) the change in internal energy of the gas, (c) the energy transfer, Q, and, (d) the final temperature.

A sample of n = 2.00 moles of monoatomic ideal gas expands adiabatically, the work done on the gas is W = -5.00 x 103 J.  The initial temperature and pressure of the gas are   Ti = 600 K and Pi = 4.05 x 105 Pa.  Calculate: a) the final temperature of the gas; b) the final pressure of the gas.  R = 8.314 J/mol K

A monatomic ideal gas initially fills a V0 = 0.45 m3 container at P0 = 85 kPa. The gas undergoes an isobaric expansion to V1 = 1.4 m3. Next it undergoes an isovolumetric cooling to its initial temperature T0. Finally it undergoes an isothermal compression to its initial pressure and volume.   1 Calculate the work done by the gas, W1, in kilojoules, during the isobaric expansion (first process).  2 Calculate the heat absorbed Q1, in kilojoules, during the isobaric expansion (first process).  3 Write an expression for the change in internal energy, ΔU1 during the isobaric expansion (first process).  4 Calculate the work done by the gas, W2, in kilojoules, during the isovolumetric cooling (second process).  5 Calculate the heat absorbed Q2, in kilojoules, during the isovolumetric cooling (second process).   6 Calculate the change in internal energy by the gas, ΔU2, in kilojoules, during the isovolumetric cooling (second process).  7 Calculate the work done by the gas, W3, in kilojoules,…

Under constant-volume conditions, 2800 J of heat is added to 1.6 moles of an ideal gas. As a result, the temperature of the gas increases by 140 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.

As shown below, a nonideal gas goes through the cycle ABCA. During the process AB, 71.5 J of heat was added to the gas. During the process BC, 8.2 J of heat was removed from the gas. Determine WABCA & QCA. WABCA = QCA P(N/m²) 10 2 2 A 4 6 8 B с 10 V (m³)

A sealed ideal gas system contains 2.0 moles of monatomic ideal gas, initially at temperature 300 K and pressure 1.2 atm. The system is allowed to expand isothermally to five times its original volume. How much heat is transferred into the system during this process? 7.09 kJ 11.2 kJ 8.03 kJ Zero 4.97 kJ

You would like to raise the temperature of an ideal gas from 295 K to 960 K in an adiabatic process. a)What compression ratio will do the job for a monatomic gas?  b)What compression ratio will do the job for a diatomic gas?