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# (a)(i) 20.57 moles of hydrogen and 5.22 moles of iodide were allowed to react to equilibrium at 4500C. At this point the mixture contained 10.22 moles of hydrogen Iodide. Show from the given data, tha

(a)(i) 20.57 moles of hydrogen and 5.22 moles of iodide were allowed to react to equilibrium at 4500C. At this point the mixture contained 10.22 moles of hydrogen Iodide. Show from the given data, tha

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EQUILIBRIUM CONSTANTS

(a)(i) 20.57 moles of hydrogen and 5.22 moles of iodide were allowed to react to equilibrium at 4500C. At this point the mixture contained 10.22 moles of hydrogen Iodide. Show from the given data, that the equilibrium constant of the reaction

H2(g)       +      I2(g)        ⇌        2HI(g)  is 61 to the nearest integer.

(ii)             If in a similar experiment, 20 moles of hydrogen and 60 moles of iodine are used.

Calculate the molar composition of the equilibrium mixture at 4500C

(b)

Hydrogen reacts with iodine according to the following equation.

H2(g)       +      I2(g)        ⇌     2HI(g)

A mixture of 0.8 moles of hydrogen and 0.6 moles of iodine was allowed to react in a sealed tube at 4500 C. At equilibrium 0.2 moles of iodine reacted.

(i)                Write the expression for the equilibrium constant KC for the reaction.

(ii)             Calculate the value of KC at 4500 C.

(c) Nitrogen monoxide combines with oxygen to form nitrogen dioxide according to equation

2NO(g)     +   O2(g)   ⇌  2NO2(g)

(i)    Write down the expression for the equilibrium constant.

(ii) 3 moles NO and 1.5 moles of oxygen were put into a vessel which was heated to 4000C. When equilibrium was established, the vessel was found to contain 0.5 moles of oxygen.

Calculate the value of KC at this temperature.

When the temperature was raised to 5000 C, the mixture in B was found to contain 25% of the initial nitrogen monoxide. Calculate the equilibrium constant at this temperature

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