Question

10) What will be the final pressure of a sample of nitrogen with a volume of 856 cm^3 at 661 torr and 25.0 ºC if it is heated to 60.0 ºC and given a final volume of 1160 cm^3?

Answer 1

The final pressure of the gas is 545.03 torr

Step-by-step explanation

Given that;

The initial volume of the gas is 856 cm^3

The initial pressure of the gas is 661 torr

The initial temperature of the gas is 25 degrees Celcius

The final temperature of the gas is 60 degrees Celcius

The final volume of the gas is 1160 cm^3

To find the final pressure of the gas, follow the steps below

Step 1; Write the general gas law

`\text{ }(P1V1)/(T1)\text{ = }(P2V2)/(T2)`

Step 2; Convert the temperatures to degrees kelvin

`\begin{gathered} \text{ t1 = 25}\degree C \\ \text{ T = t }+\text{ 273.15} \\ \text{ T = 25 + 273.15} \\ \text{ T = 298.15K} \\ \\ \text{ t2 = 60}\degree C \\ \text{ T = t }+\text{ 273.15} \\ \text{ T = 60 + 273.15} \\ \text{ T = 333.15K} \end{gathered}`

Step 3; substitute the given data into the formula in step 1

`\begin{gathered} \text{ }\frac{661\text{ }*\text{ 856}}{298.15}\text{ = }\frac{P2\text{ }*\text{ 1160}}{333.15} \\ \text{ Cross multiply} \\ \text{ 661 }*\text{ 856 }*\text{ 333.15 = P1 }*\text{ 1160 }*\text{ 298.15} \\ 188,501,600.4\text{ = 345854 P2} \\ \text{ Divide both sides by 345854} \\ (188501600.4)/(345854)\text{ = }(345854P2)/(345854) \\ \text{ P2 = 545.03 torr} \end{gathered}`

Therefore, the final pressure of the gas is 545.03 torr