Faster or Slower
Factor that increase the rate of a chemical reaction by increasing the number of effective collisions
What is temperature?
When the rate of the forward reaction equal the rate of the reverse reaction and the concentration of the reactants and products no longer changes with time
What is dynamic equilibrium?
Predict which way the following equilibrium systems will shift when the total pressure is increased.
N2(g) + O2(g) <----> 2NO(g)
What is it won't shift, moles of gas are equal?
Write an expression for the equilibrium constant for the formation of two moles of ammonia gas (NH3) from nitrogen and hydrogen in their standard states.
What is [NH3]2/[N2][H2]3?
Factor that increases rate by lowering the activation energy
What is a catalyst?
H2(g) + Br2(g) <----> 2 HBr(g)
At a certain temperature, the value of the equilibrium constant, Kc, for the reaction represented above is 2.0 x105. The Kc for
2HBr(g) <----> H2(g) + Br2(g)
What is 5.0 x 10-6
Hydrogen peroxide is decomposed as follows:
H2O2(l) <----> H2(g) + O2(g) DH = +187 kJ
Predict the direction of equilibrium shift when the temperature is increased.
What is shift to products?
Calculate the equilibrium concentrations for the reaction below if the initial [N2] = 0.80 M and the initial [O2] = .20 M
N2(g) + O2(g) <--> 2 NO(g)
Kc = 1.0 x 10-5
What is the [N2] = 0.80M
[O2]= 0.20M
[NO] = 1.3 x 10-3M
2 XY(g) ⇄ X2(g) + Y2(g) Kp = 230
A certain gas, XY(g), decomposes as represented by the equation above. A sample of each of the three gases isput in a previously evacuated container. The initial partial pressures of the gases are shown in the table below.
Gas Initial Partial Pressure (atm)
XY 0.010
X2 0.20
Y2 2.0
The temperature of the reaction mixture is held constant. In which direction will the reaction proceed?
What is to the left?
The graph of the relationship between concentration and time that is first order
What in ln conc v time?
At a certain temperature, Kc is 4.13 x 10 -2 for the equilibrium:
2 IBr (g) <--> I2(g) + Br2(g) Assume that equilibrium is established at the above temperature by adding only IBr to the reaction flask. What are the concentrations of I2 (g) and Br2 (g) in equilibrium with 0.0124 moles/liter of IBr(g)
What is 2.52 x 10-3 M?
N2(g) + 3 H2(g) <----> 2 NH3(g) DH<0
Gaseous ammonia was synthesized in the presence of a catalyst and allowed to reach equilibrium. The change in temperature that cause more ammonia to be present
What is decreasing temperature?
X(g) + 2 Q(g) ⇄ R(g) + Z(g)
Kc = 1.3 × 105 at 50oC
A 1.0 mol sample of X(g) and a 1.0 mol sample of Q(g) are introduced into an evacuated, rigid 10.0 L container and allowed to reach equilibrium at 50oC according to the equation above. The concentration of R ______ Z _______ Q
What is equal to and greater than?
Rate = k[H3AsO4] [I–] [H3O+]
What is the order of the reaction with respect to I–?
What is first order?
The rate law given:
(1) NO(g) + NO(g) --> N2O2(g) slow
(2) N2O2(g) + O2(g) --> 2 NO2(g) fast
What is rate = k[NO]2
Time(days)
0 1 2 3 4 5 6 7 … 10 … 20
%Reactant Remaining
100 79 63 50 40 31 25 20 10 1
The best description of the reaction order and 1/2 life for a reaction that was observed for 20 days.
What is 1st order and 3 days?
The equilibrium constant for the reaction:
2 NO(g) <----> N2(g) + O2(g) is 2.60 x 10-3 at 1100°C. If 0.820 mole of NO (g) and 0.223 mole each of N2 (g) and O2 (g) are mixed in a 1.00 liter container at 1100 °C, The equilibrium concentration of NO is...
What is 1.15 M?
3 O2(g) ⇄ 2 O3(g) Kc = 1.8 × 10–56 at 570 K
For the system represented above, [O2] and [O3] initially are 0.150 mol/L and 2.5 mol/L respectively. The amount of ozone ____________, since Q ___ K.
What is increases and greater than?
Rate = k[M][N]2 the rate of a certain chemical reaction between substances M and N obeys the rate law given. The reaction is first studied with [M] and [N] each 1 ´ 10–3 molar. If a new experiment is conducted with [M] and [N] each 2x10–3 molar, the reaction rate will increase by a factor of?
What is 8?
2NH3(g) <----> N2(g) + 3H2(g) At 500 K, the following concentrations were measured:
[N2] = 3.0 x 10-2 M,
[H2] = 3.7 x 10-2 M,
[NH3] = 1.6 x 10-2 M. Kc is ….
What is 5.9 x 10-3?
0.822 mole of SO3(g) is placed in a 1.00 liter container at 600 K. 36.7 % of the SO3 are decomposed when equilibrium is established.
2 SO3(g) <----> 2 SO2(g) + O2(g)
The value of Kc is ...
What is 5.05 x 10-2