Question

At constant temperature and pressure, if 0.4 mole of a gas A occupies 220 mL and x mole of B gas occupies 120 mL, what is the number of moles of gas in the container that holds them B?

Answer 1

Given:

The number of moles in gas A is,

`n_A=0.4\text{ mole}`

The volume of gas A is,

`V_A=220\text{ ml}`

The volume of gas B is,

`V_B=120\text{ ml}`

To find:

The number of moles of gas in the container that holds them B

Step-by-step explanation:

According to the ideal gas equation, as the constant temperature and pressure are constant,

`\begin{gathered} PV=nRT \\ (V)/(n)=(RT)/(P) \\ (V)/(n)=constant \end{gathered}`

So, we write,

`\begin{gathered} (V_A)/(n_A)=(V_B)/(n_B) \\ n_B=(V_Bn_A)/(V_A) \\ n_B=(120*0.4)/(220) \\ n_B=0.22 \end{gathered}`

Hence, the number of moles of gas in container B is 0.22.