1) Consider the following reaction: NH4HS(s)?NH3(g)+H2S(g) An equilibrium mixtur

Question

1) Consider the following reaction: NH4HS(s)?NH3(g)+H2S(g)

An equilibrium mixture of this reaction at a certain temperature was found to have [NH3]= 0.272M and [H2S]= 0.360M .

What is the value of the equilibrium constant (Kc) at this temperature?

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2) The reaction in Example 14.12 is carried out at the same temperature with the following initial concentrations: [H2S] = 0.100 M, [H2] = 0.100 M, and [S2] = 0.00 M. Find the equilibrium concentration of [S2].

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3) The reaction CO2(g)+C(s)?2CO(g) has Kp=5.78 at 1200 K.

Part A: Calculate the total pressure at equilibrium when 4.56g of CO2 is introduced into a 10.0-L container and heated to 1200 K in the presence of 2.19g of graphite.

Part B: Repeat the calculation of part A in the presence of 0.31g of graphite.

Thank you in advance!

Explanation / Answer

1. kc = [0.272][0.360] = 0.0979

3. CO2 + C --> 2CO
Kp = 5.78
moles CO2 = 4.56g / 44g/mole = 0.103moles
moles C = 2.19g / 12g/mole = 0.18moles
moles CO produced = 0.103 x 2 = 0.206moles CO

0.103moles CO2 initial pressure = 1.103atm
all CO2 used
0.18moles CO total pressure at end of rxn = 0.198atm

b) 0.103moles CO2, 0.025moles C
C = limiting reactant
0.103moles CO2 - 0.025moles C = 0.088moles CO2 left over
0.025moles C yields 0.05moles CO
total moles gas = 0.088 + 0.05 = 0.138moles
p = nrt/v = 1.36atm

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