# Equilibrium Worksheet I

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```					1.) The reaction between nitrogen and oxygen to form NO(g) is represented by the
chemical equation

N2 (g) + O2 (g)               2NO (g)

Equilibrium concentrations of the gases at 1500 K are 1.7x10-3 mol/L for O2 and
6.4x10-3 mol/L for N2 and 1.1x10-5 mol/L for NO. Calculate the value of Kc at 1500 K
for these data.

1.1x10-5

2.) A sealed tube initially contains 9.84x10-4 mol of H2 and 1.38x10-3 mol of I2. It is
kept at 350C until the reaction

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

comes to equilibrium. At equilibrium 4.73x10-4 moles of I2 are present. Calculate the
number of moles of H2 and HI at equilibrium and the equilibrium constant Kc for the
reaction.

H2 = 7.4x10-5 mol
HI = 1.8x10-3 mol
3.) Antimony pentachloride decomposes in a gas phase reaction at high temperatures.

SbCl5         SbCl3 (g) + Cl2 (g)

At some temperature, an equilibrium mixture in a 5.00 L container is found to contain
6.91 g of SbCl5 16.45 g of SbCl3 and 5.11 g of Cl2 Evaluate Kc.

4.49x10-2

If 10.0 grams of SbCl5 is placed in the 5.00 L container and allowed to reach
equilibrium at the same temperature, what will be the equilibrium concentrations of
all of the species?

SbCl5 = 7.90x10-4 M
Cl2 and SbCl3 = 5.90 x10-3 M

```
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