Question

A 2.5 L container holds a sample of hydrogen gas at 291 K and 180 kPa.

If the pressure increases to 350 kPa and the volume remains constant, what will the new temperature be?

Round your answer to one decimal place.

Answer 1

Answer:

The new temperature will be 565.83 K.

Explanation:

Gay Lussac's law establishes the relationship between the temperature and the pressure of a gas when the volume is constant. This law says that the pressure of the gas is directly proportional to its temperature. This means that if the temperature increases, the pressure will increase; or if the temperature decreases, the pressure will decrease.

In other words, Gay-Lussac's law states that when a gas undergoes a constant volume transformation, the ratio of the pressure exerted by the gas temperature remains constant:

$\frac{P}{T} =k$

When an ideal gas goes from a state 1 to a state 2, it is true:

$\frac{P1}{T1} =\frac{P2}{T2}$

In this case:

• P1= 180 kPa
• T1= 291 K
• P2= 350 kPa
• T2= ?

Replacing:

$\frac{180 kPa}{291 K} =\frac{350 kPa}{T2}$

Solving:

$T2=350 kPa*\frac{291 K}{180 kPa}$

T2= 565.83 K

The new temperature will be 565.83 K.