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

i can ! i just need to know what the paragraph is! : p

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.