Question

At STP, 2.8 litres of hydrogen sulphide were mixed with 1.6 litres of sulphur dioxide and the reaction occurred according to the equation

$2H_{2}S\left(g\right)+SO_{2}\left(g\right) \rightarrow 2H_{2}O\left(l\right)+3S\left(s\right)$

Which of the following shows the volume of the gas remaining after the reaction?

• A. 0.2 litres of $SO_{2}\left(g\right)$
• B. 0.4 litres of $H_{2}\left(g\right)$
• C. 1.2 litres of $H_{2}S\left(g\right)$
• D. 1.2 litres of $SO_{2}\left(g\right)$

Answer 1

Answer: (A)

So, $\text{Sol} \, \text{2} \, \text{vol} \, \text{H}_{\text{2}} \text{S} \equiv \text{1} \, \text{vol} \, \text{SO}_{\text{2}}$

or $\text{2} \text{.8} \, \text{L} \, \text{H}_{\text{2}} \text{S} \, \text{=} \, \text{1} \text{.4} \, \text{L} \, \text{SO}_{\text{2}}$

Hence, after reaction, volume of remaining $SO_{2}$

$= 1.6 - 1.4 \, \text{L}$

$= 0.2 \, \text{L}$