10.3 Problems using Kc

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10.3 Problems using Kc - Quiz 4

1.800 mol of ammonia is introduced into an evacuated 5.00 dm³ vessel and allowed to come to equilibrium. The concentration of nitrogen at equilibrium was determined to be 0.0435M. Calculate the equilibrium constant for the reaction shown below, given that the temperature remained constant at 160°C throughout.

2NH₃ ⇌ N₂ + 3H₂ *

1 point

2.45 x 10⁻³

1.87 x 10⁻³

2.14 x 10⁻³

1.31 x 10⁻³

A chemical equilibrium is established when eleven moles of hydrogen and eleven moles of iodine are mixed at a temperature of 764 K. Initially the colour of the mixture is deep purple due to the high concentration of iodine vapour. There are seventeen moles of hydrogen iodide present at equilibrium and the equilibrium is represented by the equation

H₂ + I₂ ⇌ 2HI

Calculate the value of the equilibrium constant (Kc) at 764 K.

1 point

46.24

48.56

12.56

17.92

The value of Kc for the following equilibrium reaction is 4.0 at a temperature of 373 K.

CH₃COOH + C₂H₅OH ⇌ CH₃COOC₂H₅ + H₂O

What mass of ethyl ethanoate (CH₃COOC₂H₅) would be present in the equilibrium mixture if 15g of ethanoic acid and 11.5g of ethanol were mixed and equilibrium was established at this temperature? (18)

1 point

15.6g

14.3g

18.6g

12.6g

1.50 mol of carbon monoxide and 0.500 mol of chlorine gas are introduced into an evacuated 10.0 dm³ vessel at 700 K. When the reaction reaches equilibrium, the concentration of phosgene (COCl₂) is 0.0485M. Calculate the equilibrium concentrations of CO and Cl₂ and so determine the equilibrium constant for the reaction at this temperature. The equation for the reaction is:

CO + Cl₂ ⇌ COCl₂

1 point

356

422

319

285

For the reaction

N₂ + 3H₂ ⇌ 2NH₃

three moles of nitrogen gas and nine moles of hydrogen gas were mixed in a 1 litre vessel at a temperature T. There were two moles of ammonia in the vessel at equilibrium. Calculate the value of Kc for this reaction at this temperature.

1 point

0.009

0.007

0.008

0.01

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