Question

Under improper storage, chlorine bleach decomposes and releases toxic chlorinegas, Cl2(g) What amount of toxic chlorine gas is released from 64mL of bleach at102kPa and 22°C?

Answer 1

We can use the law of ideal gases to solve this question.

The law of ideal gases is represented by the following formula:

`Pv=nRT`

Where P is the pressure, v is the volume, n is the number of moles, R is the ideal gas constant and T is the temperature.

The first step is to convert kPa to atm, °C to K and mL to L.

`102kPa\cdot(1atm)/(101.32kPa)=1atm`
`\begin{gathered} K=22+273 \\ K=295 \end{gathered}`
`64mL\cdot(1L)/(1000mL)=0.064L`

Now, we can use these values to find n, which is the amount of moles of the gas:

`\begin{gathered} n=(Pv)/(RT) \\ n=(1atm\cdot0.064L)/(295K\cdot0.082\cdot(atm\cdot L)/(mol\cdot K)) \\ n=0.00264mol \end{gathered}`

The answer is 0.00264 moles of chlorine are released.