Question

A sample of nitrogen is initially at a pressure of 1.7 kPa, a temperature of -10 C and a volume of 7.5 m3. Then the volume is decreased to 3.8 m3. the temperature is decreased to 200 K. What is the final pressure of the nitrogen gas?

A. 0.24 kPa
B. 2.55 kPa
C. 11.93 kPa
D. 232.19 kPa

Answer 1

Answer:

Option B is correct

Explanation:

The ideal gas formula can be used to find the Pressure of Nitrogen gas.

$\frac{P_{1}V_{1}}{T_{1}} = \frac{P_{2}V_{2}}{T_{2}}$

Here P is pressure, V is volume and T is temperature.

In the given question:

P₁ = 1.7 kPa

T₁ = -10°C Changing to Kelvin:  273.15 -10°C = 263.15 K

V₁ = 7.5 m^3

V₂ = 3.8 m^3

T₂ = 200 K

P₂ =?

Putting values in the formula

$\frac{1.7 *7.5 }{263.15}=\frac{P_{2*3.8}}{200}\\\frac{12.75}{263.15}=\frac{P_{2}*3.8}{200} \\0.048 = \frac{P_{2}*3.8}{200}\\=> P_{2} = \frac{0.04845*200}{3.8}\\P_{2} = 2.55 \,\,kPa$

So, Option B is correct.