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Which one of the following is NOT a key concept of the collision theory:
1.60 moles CO, 1.60 moles H2O, 4.00 moles CO2, 4.00moles H2 are found in a 8.00L container at 690oC at equilibrium.
CO (g) + H2O (g) <…..> CO2 (g) + H2 (g)
Calculate the value of the equilibrium constant.
Using the graph below for the question
Which letter shows the potential energy of the activated complex?
What is the ΔH(Heat) of the reaction?
Keq = 798 at 25oC for the reaction:
2SO2 (g) + O2 (g) <….> 2SO3 (g).
In a particular mixture at equilibrium, [SO2]= 4.20 M and [SO3]=11.0M. Calculate the equilibrium [O2] in this
mixture at 25oC
The equilibrium constant for the equilibrium below is Keq = 1.5
H2(aq) + I2(s) <—-> 2 HI(g)
Which of the following statements is true regarding this equilibrium?
I. the reaction is product favored
II. the reaction is reactant favored
III. equilibrium lies far to the right
IV. equilibrium lies far to the left
CH4(g) + 2H2S(g)) <—> CS2(g) + 4H2(g)
In which case the equilibrium position would shift to right when the following changes are made to the equilibrium system below?
2SO3(g)< —> 2SO2(g) + O2(g)
What effect does doubling the concentration of one of the reactants have on the rate of the reaction
Which of the following factors does not affect the rate of a chemical reaction?
If the pressure on the equilibrium system 2CO(g) + O2(g) <…..> 2CO2(g) is increased,
Which one of the following reactions will start with the highest rate?
The value of Keq for a system:
At equilibrium, the total amount of the product(s)
Reaction rates generally increase with an increase in temperature. Four suggested reasons are:
I. Molecules collide more frequently at higher temperatures.
II. As the temperature of a reaction increases, the activation energy for the reaction decreases.
III. The concentration of reactants will be greater at a higher temperature.
IV. The fraction of high energy molecules is greater at higher temperatures.
The correct statements are:
A lump of ignited charcoal which is glowing in air burns more vigorously when lowered into a bottle of pure oxygen. This is due to an increase in
The rate of a chemical reaction normally
Crushing a solid into a powder will increase reaction rate because:
What happens to a catalyst in a reaction?
N2(g) + 3H2(g) <……> 2NH3(g)
What is the equilibrium expression for the reaction?
The following equilibrium is readily established:
SO2Cl2 (g) <…..> SO2 (g) + Cl2 (g)
At equilibrium at 373 K, a 1.00-L reaction vessel contains 0.0106 mol of SO2Cl2 and 0.0287 mol each of SO2 and Cl2. What is Keq for the reaction at 373 K?
A reaction in which products can react to re-form reactants is
For the equilibrium system:
N2O4(g) <…..> 2 NO2(g)
Predict (based on the value of Keq) if the equilibrium will
Predict the effect of removing the heat to the equilibrium system
2H2(g) + O2(g) <……> 2H2O(g) + Heat
In the equation
, what represents the concentrations of the products?
