Hydrogen sulfide reacts with sulfur dioxide to give H2O and S, H2S + SO2 = H2O + S(solid), unbalanced. If 3.0 L of H2S gas at 760 torrs produced 4.8 g of sulfur, what is the temperature in Celsius?

To calculate temperature we have to convert grams of S to moles of S then moles of H2S then use ideal gas law to find temperature

Given

Hydrogen sulfide reacts with sulfur dioxide to give H2O and S, H2S + SO2 = H2O + S(solid), unbalanced.

Also, 3.0 L of H2S gas at 760 torr produced 4.8 g of sulfur.

Find out

We need to find out the temperature in celsius.

Solution

Let us first write the balanced Chemical equation

\(2H_{2}S + SO_{2}\rightarrow 2H_{2}O + 3S\)

Now will calculate the moles of H2S

Moles of H2S= \(4.8 g of S X \frac{1 mole of S}{32.06 g of S} X \frac{2 mole of H_{2}S}{3 mole of S}\)

Moles of H2S= 0.0998 Moles of H2S

From ideal gas law we know that

PV = nRT

P= \(760 Torr X \frac{1}{760 Torr} = 1 atm\)

T=PV / nR

T = \(\frac{1 atm X 3.o L}{o.o998 mol X 0.0826 L atm . K^{-1}mol^{-1}}\)

T = (366-273.15)

T= 90ºC

The temperature in celsius is 90º

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