Section 1
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Consider the following reaction at equilibrium 2NH3 (g) -> N2 (g) + 3H2 (g) delta H = +92.5 kJ Le Chatelier's principle predicts that adding N2 (g) to the system at equilibrium will result in _____
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Section 1
(50 cards)
Consider the following reaction at equilibrium 2NH3 (g) -> N2 (g) + 3H2 (g) delta H = +92.5 kJ Le Chatelier's principle predicts that adding N2 (g) to the system at equilibrium will result in _____
a decrease in the concentration of H2??
The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is ____ 1) SO2 (g) + 1/2 O2 (g) -> SO3 (g) 2) 2SO3 (g) -> 2SO2 (g) + O2 (g)
1/K^2
What is the coefficient of the permanganate ion when the following equation is balanced? MNO4- +Br- -> Mn2+ +Br2 (acidic solution)
2
The decomposition of n2O5 rate law is
K[N2O5]
The equilibrium constant for the reaction shown here is Kc = 1.0x10^3. A reaction mixture at equilibrium contains [A] = 1.0 x 10^-3 M. What is the concentration of B in the mixture A(g) -> B(g)
1.0M
NO3 + CO -> NO2 + CO2 Molecularity is_____ rate law is _____
2, k[NO3][CO]
Which Substance in the reaction below either appears or disappears the fastest? 4NH3 + 7O2 -> 4NO2 + 6H2O
O2
Which energy difference corresponds to the activation energy if the reverse reaction
X + y
What is the oxidation number of manganese in the MnO4- ion?
7+
The balanced half-reaction in which sulfate ion is reduced to sulfite ion is a
two electron process
The expression for Keq for the reaction below is BaS (s) + 2O2 (g) -> BaSO4 (s)
1/P O2^2
one difference between first and second-order reactions is that
the half-life of a first-order reaction does not depend on [A]0; the half-life of a second-order reaction does depend on [A]0
A reaction was found to be third order in A. Increasing the concentration of A by a factor of 3 will cause the reaction rate to
increase by a factor of 27
Which transformation could take place at the cathode of an electrochemical cell
HSO4- -> H2SO3
A burning splint will burn more vigorously in pure oxygen than in air because
oxygen is a reactant in combustion and concentration of oxygen is higher in pure oxygen than in air
Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction.... in a particular experiment at 300C, NO2 drops from .01 to .0065 M in 100 s. The rate of appearance of O2 for this period is
7x10^-5
2NH3 g -> N2 g + 3H2 g Is keq = 230 at 300C at equilibrium
Products are predominant
The solid XY decomposes into gaseous X and Y XY (s) -> X (g) + Y (g) Kp = 4.1 at 0C If the reaction is carried out in a 22.4L container, which initial amount of X and Y will result in the formation of solid XY?
Consider the following reaction at equili rium: 2CO2 (g) -> @CO (g) +O2 (g) delta H = -514 kJ Le Chatelier's principle predicts that an increase in temperature will ____
decrease the value of the equilibrium constant
Nuclear decay is ____ order and half lives ___
First, remains constant
Under constant conditions, the half-life of a fist-order reaction
does not depend on the initial reactant concentration, is constant, can be calculated from the reaction rate constant, is the time necessary for the reactant concentration to drop to half its original value (aka all of the above)
Which of the following expression is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide? N2O4 (g) -> 2NO2 (g)
[NO2]2 / N2O4
Which element is reduced in the reaction below? Fe(CO)5 (l) + 2HI (g) -> Fe(CO)4I2 (s) + CO (g) + H2 (g)
H
Which of the following reactions initially at equilibrium will form more products when the pressure is increased as constant temperature
N2 (g) + 3H2 (g) -> 2NH3 (g)
Of the following, all are valid units for a reaction rate except
mole/L
Which one of the following will change the value of an equilibrium constant?
changing temperature
If the rate law for the reaction 2A +3B -> products is first order in A and second order in B then the rate law is rate =
k[A][B]^2
The rate law of the reaction A + B -> C and positive delta h is k[A]2 which will not increase rate
Increasing the concentration of reactant b
At equilibrium
The rates of the forward and reverse reactions are equal
At 400K the equilibrium constant for the reaction Br2 (g) + Cl2 (g) -> 2BrCl (g) is Kp = 7.0. A closed vessel at 400k is charged with 1.00 atm of Br2 (g), 1.00 atm of Cl2 (g) and 2.00 atm of BrCl (g). Use Q to determine which of the statements below is true
The equilibrium partial pressure of BrCl (g) will be greater than 2.00 atm
Consider the general reaction A + B -> C + D with a Keq = 3.2 If the reaction is allowed to reach equilibrium, what is the value of delta g?
delta g will be less than 1
which of the following reactions is a redox reaction?
CU + S -> CuS
for the endothermic reaction CaCO3 (s) -> CaO (s) + CO2 (g) le chatelier's principle predicts that _____ will result in an increase in the number of moles of CO2
increasing the temperature
The purpose of the salt bridge in an electrochemical cell is to _____
maintain electrical neutrality in the half-cells via migration of ions
For the reaction 2A(g) -> B(g) the equilibrium constant is Kp = 0.76. A reaction mixture initially contains 2.0 atm of each gas. Which statement is true of the reaction mixture?
the reaction mixture will proceed towards products
how does the reaction quotient of a reaction (Q) compare with the equilibrium constant (Keq) of the same reaction
Q is the same as Keq when the reaction is at equilibrium
Which is an intermediate in the formation of XO2 from X and O2
XO
Consider the following equilibrium 2SO2 (g) + O2 (g) -> 2SO3 (g) - the equilibrium cannot be established when ____ is/are placed in a 1.0L container
.75 mol SO2 (g)
Which one of the following graphs shows the correct relationship between concentration and time for a reaction that is second order in [A]?
x axis = time, y axis = 1/[A]
the electrode at which an oxidation occurs is called the
anode
In general, as activation energy increases, reaction rate
Goes down regardless of whether the reaction is exothermic or endothermic
the gain of electrons by an element is called
reduction
Nitrosyl bromide decomposes according to the following equation 2NOBr (g) -> 2NO (g) + Br2 (g) 2NOBr (0.64 mol) was placed in a 1.00 L flask containing no NO or Br2. At equilibrium the flask contained 0.46 mol of NOBr. How many moles of NO and Br2 respectively, are in the flask at equilibrium?
0.18, 0.090
The decomposition of NH4HS is endothermic: NH4Hs (s) -> NH3(g) + H2S (g) which change to an equilibrium mixture of this reaction results in the formation of more H2S?
An increase in temperature
The overall order of a reaction is 2. The units of the rate constant for the reaction are
M-1s-1
For which of the following reactions is the value of Kp equal to Kc?
SnO2 (s) + 2H2 (g) + Sn(s) + 2H2O (g)
The graph shown below depicts the relationship between concentration and time for the following chemical reaction 2A -> C The slope of the line is equal to
-k
A catalyst can increase the rate of reaction
By providing an alternative pathway with a Lowe activation energy
The rate law for this reaction (A + B -> P) =
k[A]^2
The more ___ the value of the E^0 red, the greater the driving force for reduction
positive
Section 2
(43 cards)