Question

If a given power plant released so2 gas with a volume v of 1200 m3 at a density ρ of 2.86 kg/m3 at standard pressure and temperature, how many moles n of so2 are released? the atomic weight of sulfur is 32.07 u and the atomic weight of oxygen is 16.00 u.

Answer 1

Answer:

$\boxed{\text{52 840 mol}}$

Explanation:

Since you have the volume of the gas at STP, we can use the Ideal Gas Law to calculate the number of moles. The identity of the gas doesn't matter.

pV = nRT

n = (pV)/(RT)

Data:

p = 1 bar

V = 1200 m³ = 1.2 × 10⁶ dm³

R = 0.083 14 bar·dm³K⁻¹mol⁻¹

T = 273.15 K

Calculation:

n = (1 bar × 1.2 ×10⁶ dm³)/(0.083 14 bar·dm³K⁻¹mol⁻¹ × 273.15 K)

= 52 840 mol

The power plant releases $\boxed{\text{52 840 mol of SO}_{2}}$.