Question

A rigid plastic container holds 1.00 l methane gas at 660 torr pressure when the temperature is 22.0 degrees Celsius. How much pressure will the gas exert if the temperature is raised to 44.6 degrees Celsius?

Answer 1

To find the final pressure of the gas, we can use the combined gas law equation P1V1/T1 = P2V2/T2. By substituting the given initial values and converting temperatures to Kelvin, we can solve for P2, the final pressure.

Step-by-step explanation:

To solve this problem, we can use the combined gas law equation: P1V1/T1 = P2V2/T2. We are given the initial pressure, volume, and temperature, and we need to find the final pressure. Let's convert the initial temperature to Kelvin by adding 273.15: 22.0°C + 273.15 = 295.15 K. Similarly, convert the final temperature to Kelvin: 44.6°C + 273.15 = 317.75 K. Substitute the values into the equation:

(660 torr)(1.00 L)/(295.15 K) = P2(1.00 L)/(317.75 K)

Solving for P2, the final pressure, we get:

P2 = (660 torr)(317.75 K)/(295.15 K)

P2 ≈ 709.42 torr. Therefore, the gas will exert a pressure of approximately 709.42 torr if the temperature is raised to 44.6 degrees Celsius.

Answer 2

Answer : The final pressure of the gas will be, 710.56 torr

Explanation :

According to the Charles' Law, the pressure of the gas is directly proportional to the temperature of the gas at constant volume and the number of moles of gas.

`P\propto T`

or,

`(P_1)/(P_2)=(T_1)/(T_2)`

where,

`P_1` = initial pressure of the gas = 660 torr

`P_2` = final pressure of the gas = ?

`T_1` = initial temperature of the gas =
`22^oC=273+22=295K`

`T_2` = final temperature of the gas =
`44.6^oC=273+44.6=317.6K`

Now put all the given values in the above formula, we get the final pressure of the gas.

`(660torr)/(P_2)=(295K)/(317.6K)`

`P_2=710.56torr`

Therefore, the final pressure of the gas will be, 710.56 torr