Hydrogen sulfide reacts with sulfur dioxide to give H2O and S, H2S + SO2 = H2O + S(solid), unbalanced. If 6.0 L of H2S gas at 750 torr produced 3.2 g of sulfur, what is the temperature in Celsius?

Aug 9, 2014

The temperature is 810 °C.

Explanation:

There are four steps in this problem:

1. Write the balanced chemical equation.
2. Calculate the moles of sulfur.
3. Calculate the moles of H₂S.
4. Use the Ideal Gas Law to calculate the temperature.

1. Write the balanced chemical equation

2H₂S + SO₂ → 2H₂O + 3S

2. Calculate the moles of sulfur

Moles of S = 3.2 g S × $\left(1 \text{mol S")/(32.06"g S}\right)$ = 0.0998 mol S

3. Calculate the moles of H₂S

Moles of H₂S = 0.0998 mol S × $\left(2 \text{mol H₂S")/(3"mol S}\right)$ = 0.0665 mol H₂S

4. Calculate the temperature

$P$ = 750 Torr × $\left(1 \text{atm")/(760"Torr}\right)$ = 0.9868 atm

$P V = n R T$

$T = \frac{P V}{n R} = \left(0.9868 \text{atm" × 6.0"L")/(0.0665"mol" × 0.082 06"L·atm·K⁻¹mol⁻¹}\right)$ = 1080 K

$T$ = (1080 – 273.15) °C = 810 °C (2 significant figures)