Question

A sample of gas initially occupies 4.25 L at a pressure of 0.850 atm at 23.0°C. What will the volume be if the temperature is changed to 11.5°C, and the pressure is changed to 1.50 atm?1. 2500mL2. 7.21 x 10^3 mL3. 1.20 L4. 2.31 L5. 2.31 mL

Answer 1

`2.31\text{ L}`

Step-by-step explanation:

Here, we want to calculate the final volume

We use the general gas equation here:

`(P_1V_1)/(T_1)\text{ = }(P_2V_2)/(T_2)`

P1 is the initial pressure which is 0.850 atm

V1 is the initial volume which is 4.25 L

T1 is the initial temperature which is (23 + 273.15 = 296.15 K)

P2 is the final pressure which is 1.50 atm

V2 is the final volume which is unknown

T2 is the final temperature (11.5 + 273.15 = 284.65 K)

Substituting the values, we have:

`\begin{gathered} \frac{0.850\text{ }*4.25}{296.15}\text{ = }(1.50* V_2)/(284.65) \\ \\ V_2\text{ = }\frac{284.65\text{ }*0.850*4.25}{1.5*296.15} \\ \\ V_2\text{ = 2.31 L} \end{gathered}`