A sealed container of nitrogen gas is at 1000.0 kPa pressure and at a temperature of 20.00 °C. The container is left in the sun, and the temperature of the gas increases to 50.00 °C. What is the new pressure in the container, assuming the volume remains constant? A. 1102 kPa B. 1182 kPa C. 1208 kPa D. 1244 kPa

P₂ = 1102 Kpa

Explanation:

Given data:

Initial pressure = 1000.0 Kpa

Initial temperature = 20.0°C

Final temperature = 50.0°C

Final pressure = ?

Solution:

Initial temperature = 20.0°C (20+273 = 293 K)

Final temperature = 50.0°C (50+273 = 323 K)

According to Gay-Lussac Law,

The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.

Mathematical relationship:

P₁/T₁ = P₂/T₂

Now we will put the values in formula:

1000 Kpa / 293 K = P₂/323 K

P₂ = 1000 Kpa × 323 K / 293 K

P₂ = 323000 Kpa. K /293 K

P₂ = 1102 Kpa

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