A1.75-l container filled with co2 gas at 25°c and 225 kpa pressure springs a leak. when the container is re-sealed, the pressure is 185 kpa and the temperature is 10°c. how many moles of gas were lost? a.0.463 mol b.0.0213 mol c.0.561 mol d.2.16 mol

The ideal gas law is
pY = nRT
where
p = pressure
V = volume
T =  absolute temperature
n = number of moles
R =  gas constant, 8.314 J*(mol-K)

Therefore, the number of moles is


The given volume is
V = 1.75 L = 1.75 x 10⁻³ m³

State 1:
T₁ = 25 C = 25+273 = 298 K
p₁ = 225 kPa = 225 x 10³ N/m²

State 2:
T₂ = 10 C = 283 K
p₂ = 185 kPa = 185 x 10³ N/m²

The loss in moles of gas from state 1 to state 2 is


V/R = (1.75 x 10⁻³ m³)/(8.314 (N-m)/(mol-K) = 2.1049 x 10⁻⁴ (mol-m²-K)/N
p₁/T₁ = (225 x 10³)/298 = 755.0336 N/(m²-K)
p₂/T₂ = (185 x 10³)/283 = 653.7102 N/(m²-K)

Therefore
Δn = (2.1049 x 10⁻⁴ (mol-m²-K)/N)*(755.0336 - 653.7102 N/(m²-K))
     = 0.0213 mol

b.  0.0213 mol

Adozen is 1221/12 = 1.751.75 x 12 = 21therefore, 1.75 is the answer.

Sorry i dont understand the question can you rephase it?