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- Show that = T/p for an ideal gas.A piston reversibly and adiabatically contracts 3.88 moles of ideal gas to one-tenth of its original volume, thenexpands back to the original conditions. It does thisa total of five times. If the initial and final temperatures both are 27.5C, calculatea thetotal work andb thetotal U forthe overall process.A sample of an ideal diatomic gas is compressed adiabatically and reversibly to double its initial pressure. By what percentage does its absolute temperature change in a the low-temperature limit and b the high-temperature limit?
- 1 mol of N2 gas in a volume of 300 K and 2 L undergoes an isothermal reversible expansion up to 20 L final volume. In this case, calculate the work considering that the gas a) behaves ideally b) behaves in accordance with the van der Waals equation. Calculate the percent error in work when the ideal gas equation is used instead of the van der Waals equation.How would an ideal gas (where dU=Cv(dt) is always true) undergoing isothermal reversible expansion be represented by the equation for the First Law? Think about what is changing in order to do work. Which term(s) is/are now zero?One mole sample of an ideal, monoatomic gas initially has a molar volume of 24.45 L/mole at 1 bar and 298.2 K. It was expanded adiabatically and reversibly to 187.8K where the molar volume increased to 48.90 L/mole. How many KJ of work is involved in the process? Express answer in three significant figures
- A 2.45 mole quantity of methane gas initially at 315K and a pressure of 12.4atm expands to a final pressure of 0.925atm which is also the constant ext pressure. The expansion occurs adiabatically and reversibly. calculate q, w, deltaH and deltaU1 mol of N2 gas in a volume of 300 K and 2 L undergoes an isothermal reversible expansion up to 20 L final volume. In this case, calculate the work by assuming that the gas a) behaves ideally b) behaves in accordance with the van der Waals equation. Calculate the percent error in work when using the ideal gas equation instead of the van der Waals equationCalculate ∆U and ∆H in heating 55.4 g of Xe from 300 K to 450 K. Assume the heat capacities atconstant volume and constant pressure to be independent of temperature and ideal gas behavior
- Calculate the minimum constant Pext required for an isothermal compression of 1.5 mol of a vander Waals gas from 5.00 L to 0.850 L. Then, calculate w, q, and ΔU for the compression. a= 0.245 atm mol-2 L2, b=0.005 L mol-1. T=300K1 mol of N2 gas in a volume of 300 K and 2 L undergoes an isothermal reversible expansion up to 20 L final volume. In this case, the gas Calculate the work, a) considering that it behaves ideally, b) assuming that it behaves in accordance with the van der Waals equation. Calculate the percent error in work when the ideal gas equation is used instead of the van der Waals equation.One mole of a monatomic ideal gas goes through the cycle indicated in the figure according to stages 1,2 and 3 and involving states A, B and C. Assuming that all stages are reversible. CV = 3 / 2R. Calculate Q, W, ΔU and ΔH for each process and for the cycle.
