Question

0.1 mol of ethane gas and 0.3 mol of oxygen gas are taken in a flask at 27 degree C and 1.0 atm pressure and sealed. Now the flask is heated to 1000K where the following reaction occurs quantitatively. Calculate the partial pressure of each component at the end of reaction. 2 C2H6 + 5 O2 = 2 CO2 + 3 H2O

Answer 1

Answer:

Moles of methane = 0.2

Moles of hydrogen = 0.3

Volume = 10 L

Temperature = 25 + 273 = 298 K

PV = nRT

P = VnRT

Partial pressure of methane = 100.2×0.0821×208

Partial pressure of methane = 0.489 atm

Partial pressure of hydrogen = 100.3×0.0821×208

Partial pressure of methane = 0.734 atm

Total Pressure of the gaseous mixture = 0.489 atm + 0.734 atm =1.22 atm

mark me as brainliast