Answer to Question #251336 in Molecular Physics | Thermodynamics for ellea

Question #251336

2 C2H6(g) +7 O2(g) = 4 CO2(g) + 6 H2O(g)

1. Calculate the volume in liters of CO2 at STP, that could be produced from 7.25 g C2H6.

2. Calculate the volume of O2 at 100oC and 1.25 atm, that would react with 7.52g of C2H6

1
Expert's answer
2021-10-14T18:39:02-0400

1. M(C2H6) = 30.07 g/mol

n(C2H6) =7.2530.07=0.241  mol= \frac{7.25}{30.07} = 0.241 \;mol

According to the reaction equation

n(CO2) = 2n(C2H6) =2×0.241=0.482  mol= 2 \times 0.241 = 0.482 \;mol

At STP one mole of any gas occupies 22.4 L.

V(CO2) =22.4×0.482=10.80  L= 22.4 \times 0.482 = 10.80 \;L

2. n(C2H6) =7.5230.07=0.25  mol= \frac{7.52}{30.07} = 0.25 \;mol

According to the reaction equation

n(O2) =72= \frac{7}{2} n(C2H6) =72×0.25=0.875  mol= \frac{7}{2} \times 0.25 = 0.875 \;mol

Ideal gas law:

pV=nRTp=1.25  atmT=100+273=373  KpV=nRT \\ p = 1.25 \;atm \\ T = 100 +273 = 373 \;K

R = 0.08206 L×atm/mol×K

V(O2)=nRTp=0.875×0.08206×3731.25=21.42  LV(O_2) = \frac{nRT}{p} \\ = \frac{0.875 \times 0.08206 \times 373}{1.25} \\ = 21.42 \;L


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