A 610-g quantity of an ideal gas undergoes a reversible isothermal compression at a temperature of The compression reduces the volume of the gas from initially,to finally.The molecular mass of the gas is and the ideal gas constant is R = 8.314 J/(mol ∙ K).The entropy change for the gas is closest to

Question

A 610-g quantity of an ideal gas undergoes a reversible isothermal compression at a temperature of  The compression reduces the volume of the gas from  initially,to  finally.The molecular mass of the gas is  and the ideal gas constant is R = 8.314 J/(mol ∙ K).The entropy change for the gas is closest to

Quizplus · Accepted Answer

Since the process is isothermal, the temperature remains constant throughout the process. Therefore, we can use the following equation to calculate the entropy change:

ΔS = nR ln(Vf/Vi)

where n is the number of moles of gas, R is the ideal gas constant, and Vf and Vi are the final and initial volumes, respectively.

To find the number of moles of gas, we can use the following equation:

n = m/M

where m is the mass of the gas and M is the molecular mass of the gas.

Substituting the given values, we have:

n = 610 g / 11eab929_2970_b07c_99e6_3fadec80995d_TB4470_11 g/mol = 55.45 mol

ΔS = 55.45 mol x 8.314 J/(mol*K) ln(11eab929_2970_b07b_99e6_b3fefecc366e_TB4470_11/11eab929_2970_896a_99e6_b38d1861c28a_TB4470_11)

ΔS = -99 J/K

Therefore, the entropy change for the gas is closest to -99 J/K, which is choice A.

A 610-G Quantity of an Ideal Gas Undergoes a Reversible