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NH4HS(s) <==> NH3(g) + H2S(g) ΔHRXN > 0
A sealed rigid vessel contains NH4HS(s) in equilibrium with NH3(g) and H2S(g)as represented by the equation above.
Which of the following changes will increase the amount of NH4HS(s) in the vessel?
Removing a small amount of NH3(g)
Removing a small amount of H2S(g)
Adding He gas to the vessel
Lowering the temperature
HgO(s) + 4 I− + H2O ⇄ HgI42− + 2 OH− ∆H < 0
Consider the equilibrium above.
Which of the following changes will increase the concentration of HgI42−?
Adding 6 M HNO3
Increasing the concentration of OH−
Increasing the mass of HgO present
Increasing the temperature
What is the effect of increasing the pressure on the following reaction:
2NO + O2 ---> 2NO2?
The yield of NO2 increases
The yield of NO2 decreases
The reaction is slower
The concentration of O2 increases.
Forward reaction is favored when
K is less than 1
K is greater than 1
K is equal to zero
When the reaction is reversed,
K for the reverse equals K for the forward reaction
K for the reverse is the negative of K for the forward reaction
K for the reverse is the reciprocal of K for the forward reaction
When two reactions are added, then their equilibrium constants are:
multiplied
added
subtracted
none of the above
The reaction 2 SO2(g) + O2(g) ↔ 2 SO3(g) has an equilibrium constant of K1. What is the K value for the reaction
SO3(g) ↔ SO2(g) + 1/2 O2(g)?
1/2 K1
1/K1
(1/K1)1/2
K11/2
What is the value for the reaction N2(g) + 2O2(g) ↔ N2O4(g) in terms of the K values for the following reactions:
1/2 N2(g) + 1/2 O2(g) ↔ NO(g) K1
2 NO(g) + O2(g) ↔ N2O4(g) K2
K1 + K2
K12 + K2
2 K1 x K2
K12 x K2
If the solubility of MgCO3 is represented by s, which expression is equal to the Ksp?
2s
s2
4s2
4s3
If the solubility of Ag2CO3 is represented by s, which expression is equal to the Ksp?
2s
s2
4s2
4s3
For the reaction,
CO2(g) + 4 H2(g) ↔ CH4(g) + 2 H2O(g),
K = 8.2 x 1019 at 25°C.
Initially CO2(g) and H2(g) are 1.0atm at 25°C in an evacuated container, which substance will have the highest pressure when the system is at equilibrium?
CO2(g)
H2(g)
CH4(g)
H2O(g)
C(s) + H2O(g) ↔ H2(g) + CO(g)
ΔH° = +131 kJ/mol
Which stress will INCREASE the value of the equilibrium constant, K?
some C(s) is added
the temperature of the system is increased
the container is compressed
the temperature of the system is decreased
C(s) + H2O(g) ↔ H2(g) + CO(g)
ΔH° = 131 kJ/mol
Which change will increase the [H2(g)] without affecting the value of K?
some C(s) is added
the temperature is increased
the container is compressed
some H2O(g) is added
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