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32 questions
Given the Kc for a forward reaction, how can you find Kc for the reverse reaction?
Divide Kc by 1
Divide 1 by Kc
Square Kc
Take the square root of Kc
For the reaction...
heat + N2 + O2 ↔ 2NO
If heat is added to the chemical system, the equilibrium will shift _______.
left
right
left and right
neither left nor right
2SO2(g)+O2(g)⇌2SO3(g)
Decreasing the volume of container will
shift equilibrium right
shift equilibrium left
change K
have no change
The following reaction :
SO2 (g) + NO2 (g) <=> SO3 (g) + NO (g)
had reached a state of equilibrium, was found to contain
0.40 mol L-1 SO3 , and 0.30 mol L-1 NO,
0.15 mol L-1NO2 , and 0.20 mol L-1 SO2.
Calculate the equilibrium constant for this reaction.
4.0
0.42
0.25
1.0
When 0.40 mole of SO2 and 0.60 mole of O2 are placed in an evacuated 1.00–liter flask, the reaction represented below occurs.
2SO2 (g) + O2 (g) ↔ 2SO3 (g)
After the reactants and the product reach equilibrium and the initial temperature is restored, the flask is found to contain 0.30 mole of SO3. Based on these results, the equilibrium constant, Kc, for the reaction is
20
10
6.7
2.0
In which of the following systems would the number of moles of the substances present at equilibrium NOT be shifted by a change in the volume of the system at constant temperature?
CO(g) + NO(g) ↔ CO2(g) + ½N2(g)
N2(g) + 3H2(g) ↔ 2NH3(g)
N2(g) + 2O2(g) ↔ 2 NO2(g)
NO(g) + O3(g) ↔ NO2(g) + O2(g)
H2(g) +I2(g) ↔ 2HI(g)
All gases begin with an initial concentration of 2.0 M. Equilibrium is established, and the concentration of HI is known to be 4.8 M. What is the value of the equilibrium constant?
1.2
2.4
32
64
Consider the following equation: CO(g) + 2H2(g) ⇌ CH3OH(g) + Heat
Which of the factors below would decrease the concentration of CH3OH at equilibrium?
adding CO
incresing H2
decrease in the temperature
increasing the temperature
(Calculator Allowed) What is [H2O] if K = 1.2,
[CO2] = 0.846M, & [CH4]= 0.0713M?
4CuO(s)+CH4(g)↔CO2(g)+4Cu(s) +2H2O(g)
0.101 M
0.318 M
0.0102 M
3.77 M
COCl2(g) ⇄ CO(g) + Cl2(g)
APMCQ: COCl2(g) decomposes according to the equation above. When pure COCl2(g) is injected into a rigid, previously evacuated flask at 690 K, the pressure in the flask is initially 1.0 atm. After the reaction reaches equilibrium at 690 K, the total pressure in the flask is 1.2 atm. What is the value of Kp for the reaction at 690 K?
0.2
0.05
0.8
1.0
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