Can you help me fine what is incorrect with these equations/statements? Thanks \

Question

Can you help me fine what is incorrect with these equations/statements? Thanks

"The heat capacity of a diatomic ideal gas at constant volume is 9/2 nR because the translational, vibrational and rotational degrees of freedom each contribute 3 Times 1/2 nR to the heat capacity", Explain why this statement is incorrect. For the reaction C6H12O6 (s) + 602 (g) rightarrow 6CO2 (g) + 6H2O What is the one major mistake in this calculation? One mole of a monoatomic ideal gas is heated reversibly from 10 degree C to 20 degree C in a constant volume container. Why is it incorrect to use the formula Delta S = nR ln to calculate the entropy change for this reversible process? 18.02 g of liquid water is enclosed under a frictionless and weightless piston at 3 100 degree C and 1 atm pressure. The pressure above the piston is lowered slightly below 1 atm, and the water inside the piston allowed to vaporize (and expand) isothermally until all of the liquid has been converted into gas. Why is it incorrect to use the formula dq = CdT to calculate the heat absorbed during this process (besides the fact that the volume is not constant)?

Explanation / Answer

A) Heat capacity is not related to the degrees of freedom.

B)there is no any mistake in the calculation

C)because of the volume is constant, in the formula there is variation in volume

D)because the formula is for adiabatic change. but in the problem the condition is isothermal.

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