WorksheetsEquilibrium Q Vs. K
Total questions: 12
Worksheet time: 18mins
Write the reverse reaction for NH4Cl (s) ⇌ NH3 (g) + HCl (g)
NH4Cl (s) ⇌ NH3 (g) + HCl (g)
NH3 (g) + HCl (g) ⇌ NH4Cl (s)
NH3 (g) + HCl (g) ⇌ NH3 (g) + HCl (g)
NH4Cl (s) ⇌ NH4Cl (s)
How can you tell that a reaction is a EQUILIBRIUM Reaction?
There are NO observable changes
The system is open
Forward and reverse processes occur simultaneously AND at the same rate
The system is closed
Draw the graph of a equilibrium reaction.
A + B ⇄ C + D
What is the formula for Kc? Kc=
[C]^c[D]^d/[A]^a[B]^b
[A]^a[B]^b/[C]^c[D]^d
When the equation is reversed, the value of K is inverted.
When the coefficients in a balanced equation are multiplied by a common factor, the equilibrium constant is raised to the power of the corresponding factor.
When the coefficients in a balanced equation are divided by a common factor, the corresponding root of the equilibrium constant is taken.
When individual equations are combined, their equilibrium constants are multiplied to obtain the equilibrium constant for the overall reaction.
What happens to the equilibrium constant when the coefficients in a balanced equation are multiplied by a common factor?
It remains the same
It decreases
It is divided by the factor
It is raised to the power of the corresponding factor
What happens to the value of K when the equation is reversed?
It remains the same
It is halved
It is squared
It is inverted
How are equilibrium constants for individual equations combined to obtain the equilibrium constant for the overall reaction?
Added
Subtracted
Multiplied
Divided
What is done to the equilibrium constant when the coefficients in a balanced equation are divided by a common factor?
Multiplied
Subtracted
Square Root
Divided
What is the formula for Kp? Kp=
[B]^b[D]^d/[C]^c[A]^a
[C]^c[D]^d/[A]^a[B]^b
[A]^a[B]^b/[C]^c[D]^d
[C]^c[A]^a/[B]^b[D]^d
What is the equilibrium constant in N2(g) + 3H2(g) ⇄ 2NH3(g)?
[NH3] = 3.1×10-2 mol L-1
[N2] = 8.5×10-1 mol L-1
[H2] = 3.1×10-3 mol L-1
3.0 x 10^4
1.5 x 10^4
2.5 x 10^4
3.8 x 10^4
What is the value of the equilibrium constant for the reaction 2NO2(g) ⇄ N2O4(g) at 100oC? N2O4(g) ⇄ 2NO2(g) Kc = 0.212 @ 100oC
What is the value of the equilibrium constant for the reaction, 2I2(g) + 2Cl2(g) ⇄ 4ICl(g)?
½I2(g) + ½Cl2 (g) ⇄ ICl(g)
Kc = 4.54 x 10^2 @ 25oC?
4.25 x 10^10
Calculate the value of Kc for the reaction: 2NO(g) + Br2(g) ⇄ 2NOBr (g) using the following information. 2 NO(g) ⇄ N2(g) + O2(g)
Kc1 = 1 x 10^30
N2(g) + Br2(g) + O2(g) ⇄ 2NOBr(g)
Kc2 = 2 x 10^-27
Calculate the value of Kc for the reaction: 2 N2O(g) + 3 O2(g) ⇄ 2N2O4(g) using the following information.
2N2(g) + O2(g) ⇄ 2N2O(g) Kc = 1.2 x 10-35
N2O4(g) ⇄ 2NO2(g) Kc = 4.6 x 10-3
½N2(g) + O2(g) ⇄ NO2(g) Kc = 4.1 x 10-9
1.1x10^6
1.1x10^-6
2.2x10^-6
2.2x10^6
What is known about the equation when Q > K
Reactants are greater than the products
Products are greater than the reactants
Shifts to the right (products)
Shifts to the left (reactants)
What is known about the equation when Q = K
System is not real
System is at equilibrium
No shift will occur
System is not at equilibrium
What is known about the equation when Q > K
Reactants are greater than the products
Products are greater than the reactants
Shifts to the right
Shifts to the left
What is the difference between Q and K?
K is the equilibrium constant
K is the reactant quotient
Q is the reactant quotient
Q is the equilibrium constant
