Question

In a
to dm² flask ,4.3 moles of H₂ and 1.97
moles of Is are heated together at 773k .. At
equilibrium 2.4 moles of HI OR ferend to be present
,
calculate equilibrium constant 'ke of the reaction.​

Answer 1

Answer:

Moles of methane = 0.2

Moles of hydrogen = 0.3

Volume = 10 L

Temperature = 25 + 273 = 298 K

PV = nRT

P =

V

nRT

Partial pressure of methane =

10

0.2×0.0821×208

Partial pressure of methane = 0.489 atm

Partial pressure of hydrogen =

10

0.3×0.0821×208

Partial pressure of methane = 0.734 atm

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

I hope fully answer

Answer 2

Answer:

hydrogen 2×45is 0098

oxygen is457789