Pure hydrogen sulphide is stored in a tank of 100 litre capacity at 20ºC and 2 atm pressure. The mas — States of Matter and Gaseous State Chemistry Question

💡 Solution & Explanation

# Solution: Mass of Pure Hydrogen Sulfide **Given Data:** - Volume: $V = 100$ L - Temperature: $T = 20°C = 293$ K - Pressure: $P = 2$ atm - Molar mass of $H_2S$: $M = 2(1) + 32 = 34$ g/mol **Step 1: Apply Ideal Gas Law** $$PV = nRT$$ where $n$ = number of moles, $R = 0.0821$ L·atm/(mol·K) **Step 2: Solve for moles** $$n = \frac{PV}{RT} = \frac{2 \times 100}{0.0821 \times 293}$$ $$n = \frac{200}{24.08} = 8.31 \text{ mol}$$ **Step 3: Calculate mass** $$\text{Mass} = n \times M = 8.31 \times 34 = 282.5 \text{ g} \approx 283 \text{ g}$$ **Answer:** The mass of $H_2S$ is approximately **283 g** (or **0.283 kg**) This uses the ideal gas law at standard conditions, which is valid for $H_2S$ gas at 2 atm and room temperature.