Question

a) hydrogen sulphide gas burns in air to give water n sulphur dioxide :- 2H2S (g) + 3O2(g) --------->2H2O(l) + 2SO2(g)......
b) hydrogen sulphide gas reacts with oxygen gas to form solid sulphur n liquid water :- 2H2S (g) + O2 ---------> 2S(s) + 2H2O (l)....
In these two EQ. Why there r products of these two r different but reactants r same????? ...

Answer 1

The temperature of the gas is 90 °C.

Explanation:

You must convert

grams of S→moles of S→moles of H2S

and then use the Ideal Gas Law to find the temperature of the H2S.

1. Write the balanced equation.

The balanced equation is

2H2S+SO2→2H2O+3S

2. Calculate the moles of H2S.

moles of H2S=4.8g S×1mol S32.06g S×2 mol H2S3mol S=0.0998 mol H2S

3. Use the Ideal Gas Law to calculate the temperature of the H2S.

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯∣∣aaPV=nRTaa∣∣−−−−−−−−−−−−−−−

P=760Torr×1 atm760Torr= 1.00 atm

T=PVnR=1.00atm×3.0L0.0998mol×0.082 06L⋅atm⋅K-1mol-1=366 K

T=(366 – 273.15) K=90 °C

Note: The answer can have only 1 significant figure, because the Kelvin temperature has only 2 significant digits. If you need more precision, you will have to recalculate.