The equilibrium constant is 8.8 x 102 at a particular temperature for the reaction: H2(g) + I2(g) ⇌ 2HI(g) Use this information to decide what will happen, given the following sets of initial conditions: Will the reaction shift to the left, to the right or will the system be at equilibrium? A 4.0 L flask contains 1.17 mol H2, 0.083 mol I2 and 8.11 mol HI. A 2.0 L flask contains 0.0455 mol H2, 0.012 mol I2 and 0.693 mol HI. PH2 = 0.5380 torr, PI2 = 0.066 torr, PHI = 5.59 torr PH2 = 0.47 torr, PI2 = 0.061 torr, PHI = 5.99 torr

when the balanced equation for the reaction is:

          H2(g) + i2(g)⇄ 2Hi

initial    0.5      0.5        X

            -X        -X         +X

Final (0.5-x)    (0.5-x)   2X

by substitution at the Kc formula:

Kc= [Hi]^2 / [H2] * [i2]

53.3 = (2X)^2 / (0.5-X) (0.5-X)by taking the square route

√53.3 = 2X / (0.5-X)

∴X = 0.39 m

∴[Hi] = 0.39 m

the correct answer is option d

explanation:

i was wrong its d because they dont use cm when calculating square roots

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !