Question

A gas cylinder contains nitrogen gas at 10.0 atm pressure and a temperature of 20. °C. The cylinder is left in the sun, and the

*amperature of the gas increases to 50. °C. What is the pressure in the cylinder?

Answer 1

Pressure = 10.9 atm

Step-by-step explanation:

According to Charles's law, the volume of a gas is directly proportional to its temperature, provided the pressure remains constant. Therefore, if the temperature of a gas increases, the volume increases proportionally.

Now, since the cylinder is rigid, the volume of the gas inside remains constant. Therefore, if the temperature of the gas increases, the pressure must also increase to maintain the same volume.

We can use the combined gas law to solve this problem. The combined gas law relates the pressure, volume, and temperature of a gas:

(P1V1)/T1 = (P2V2)/T2

where P1, V1, and T1 are the initial pressure, volume, and temperature of the gas, and P2, V2, and T2 are the final pressure, volume, and temperature of the gas.

We can rearrange the equation to solve for P2:

P2 = (P1 x T2 x V1) / (T1 x V2)

Substituting the given values, we get:

P2 = (10.0 atm x (273 + 50) K x V1) / ((273 + 20) K x V1)

The volume of the gas cancels out, so we get:

P2 = (10.0 atm x 323 K) / 293 K

P2 = 10.9 atm (rounded to one decimal place)

Therefore, the pressure in the cylinder is approximately 10.9 atm when the temperature of the gas inside is 50 °C.