A monatomic ideal gas with volume 0.195 L is rapidly compressed, so the process can be considered adiabatic. If the gas is initially at 1.01  105 Pa and 3.00  102 K and the final temperature is 455 K, find the work done by the gas on the environment, Wenv. Wenv =  J

A sample of an ideal gas is expanded to twice its original volume of 1.00 m³ in a quasi-static process for which P=aV², with α= 4.53 atm/m6, as shown in the P-V plot below. How much work is done on the expanding gas? P Les P=av² 1.00 m³ 2.00 m³

A monatomic ideal gas at 27.0°C undergoes a constant volume process from A to B and a constant-pressure process from B to C.        where P1 = 2.20, P2 = 4.40, V1 = 2.20, and V2 = 4.40.     Find the total work done on the gas during these two processes.

Assume that 9.63 moles of a monatomic ideal gas expand adiabatically, lowering the temperature from 388 to 262 K. Calculate (a) the work done by the gas (including the algebraic sign) and (b) the change in the gas's internal energy.

A 1.00 mole of helium gas is held P (atm) at a constant pressure of 1 atm and contracts from an initial volume of 50 liters to a final volume of 10 liters shown with points B and C in the Figure. This is an example of an isobaric process. a) How much work, W, does the gas do as it contracts? b) What is the change in the (internal) energy, U, of the gas? c) How much heat, Q, has been transferred to the gas during this process? 5 C 10 d) Verify that the 1st law of thermodynamics is satisfied. 1 atm=1.01x105 N/m², 1 liter=0.001 m³, NA-6.02x1023 mol¹, ks=1.38x10 23 J/K. B 50 V (liters)

ANSWER ONLY QUESTION B AND C, THANK YOU . QUESTION A ALREADY ASKED BEFORE

The gas cycled as shown. Calculate the heat supplied to the gas during the process C-A when QA-B = 20.0 J is the heat supplied during the process A-B, the process B-C is adiabatic and the total work done by the gas done during the cycle is 15.0 J?

A cylinder containing n mol of an ideal gas undergoes an adibatic process. Starting with dW = pdV and using the condition pVY = constant, show that the work done by the gas: 1 W × (p;V; - PfV¢) %3D Starting from the first law of thermodynamics in differential form, prove that the work done by the gas is n×Cy(T; - Tf).

Please help me

Please use the W=nRTln(V2/V1) equation.