Determine the work, in kJ, necessary to compress \(2 \mathrm{~kg}\) of air from \(100 \mathrm{kPa}\) to 4000 \(\mathrm{kPa}\) if the temperature is held constant at \(300^{\circ} \mathrm{C}\). a) \(-1210\) c) \(-932\) b) \(-1105\) d) \(-812\)

Short Answer

Expert verified
Answer: The work done is approximately -1105 kJ.

Step by step solution

01

Convert the temperature to Kelvin

First, we need to convert the given temperature from Celsius to Kelvin. The conversion is done by adding 273.15 to the given temperature. \(T(K) = T(^{\circ}C) + 273.15 = 300 + 273.15 = 573.15 \mathrm{K}\)
02

Calculate the number of moles of air

To calculate the number of moles, we use the ideal gas equation. First, we need to calculate the volume of the air at the initial pressure using: \(V_i = \dfrac{n_iRT}{P_i}\) We also need to find the specific gas constant of air, which is \(R = 0.287 \mathrm{~kJ/kg \cdot K}\). Since we are given the mass of the air, we can use this to find the number of moles (\(n_i\)) of the air: \(n_i = \dfrac{m}{M_{air}}\) Here, \(m = 2 \mathrm{~kg}\) and \(M_{air} = 29 \mathrm{~g/mol}\). Now, we can calculate: \(n_i = \dfrac{2 \times 10^3 \mathrm{~g}}{29 \mathrm{~g/mol}} = 68.97 \mathrm{~mol} \)
03

Determine the initial and final volumes

Now we can determine the initial and final volumes of the air using the ideal gas equation: \(V_i = \dfrac{n_iRT}{P_i} = \dfrac{68.97 \cdot 0.287 \cdot 573.15}{100} = 10.23 \mathrm{~m^3} \) \(V_f = \dfrac{n_iRT}{P_f} = \dfrac{68.97 \cdot 0.287 \cdot 573.15}{4000} = 0.2548 \mathrm{~m^3}\)
04

Calculate the work done

Now, we can calculate the work done using the formula for work in an isothermal process: \(W = nRT \ln\left(\dfrac{V_f}{V_i}\right) = 68.97 \cdot 0.287 \cdot 573.15 \cdot \ln\left(\dfrac{0.2548}{10.23}\right) = -1104.97 \mathrm{~kJ}\) Rounding to the nearest whole number, the work done is \(-1105\) kJ. So, the correct answer is \(\boxed{\text{(b) }-1105}\).

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