Question

When coal is burned, the sulfur present in coal is converted to sulfur dioxide (SO2), which is responsible for the acid rain phenomenon. S(s) + O2(g) → SO2(g) If 4.82 kg of S are reacted with oxygen, calculate the volume of SO2 gas (in mL) formed at 29°C and 1.16 atm.

. Calculate the mass in grams of hydrogen chloride produced when 5.65 L of molecular hydrogen measured at STP reacts with an excess of molecular chlorine gas.

H2(g) + Cl2(g) → 2HCl(g)

Answer 1

S(s) + O2(g) → SO2(g)

molar mass of S = 32.065 gm/mole that mean 1 mole of sulphur = 32.065 gm

molar mass of SO₂ = 64.066 gm / mole that mean 1 mole of SO₂ = 64.066 gm

According to reaction 1 mole of sulphur produce 1 mole of SO₂ that mean 32.065 gm of sulphur produce 64.066 gm of SO₂ then 4.82 kg sulphur produce 64.066 4.82 /32.065 = 9.63 kg of SO₂

9.63 kg = 9630 gm

9630/64.066 = 150.31 mole

29⁰C = 302.15 K

PV = nRT

then V = nRT/ P

V = 150.31 0.08205 302.15 / 1.16 = 3726.396 L = 3726396 ml

H2(g) + Cl2(g) → 2HCl(g)

according to reaction 1 mole of H₂ produce 2 mole of HCl

at STP 1 mole gas occupy volume 22.414 L then 5.65 L = 5.65/22.414 = 0.252 mole

according to reaction 1 mole of H₂ produce 2 mole of HCl then 0.252 mole H₂ produce 0.504 mole of HCl

1 mole of HCl = 36.4609 gm then 0.504 mole of HCl = 36.4609 0.504 = 18.376 gm

18.376 gm HCl produced.