Chemistry 1027A/B Lecture Notes - Gas Constant, Inert Gas, Equilibrium Constant

47 views6 pages

bluellama358

3 Jul 2013

School

Department

Course

Professor

For unlimited access to Class Notes, a Class+ subscription is required.

Document Summary

The equilibrium constant expression: a general equilibrium reaction is written as: aa + bb cc + dd reactants products, the general form of the equilibrium constant expression for this reaction using concentrations is: [a]a[b]b: the concentration of any solid, or of any solvent, is considered to be constant and is therefore omitted from the equilibrium constant expression. Le ch telier"s principle: equilibrium can be disturbed in several ways: Adding or removing one of the reactants or products. Changing the pressure of a gaseous system. Increasing temperature has the same effect as increasing the amount of one of the reactants; results in a shift of the equilibrium to the right, increasing the amounts of products and increasing the value of k. Increasing temperature has the same effect as increasing the amount of one of the product; results in a shift of the equilibrium to the left, increasing the amounts of the reactants and decreasing the value of k.

Related Questions

1) If the temperature of an endothermic reaction at equilibriumcould be increased instantaneously, what would be the instantaneouseffect on Q and K before equilibrium was againachieved?

a.	Q would increase and K would stay thesame.
b.	Q would decrease and K would stay thesame.
c.	Q would stay the same and K wouldincrease.
d.	Q would stay the same and K woulddecrease.
e.	Both Q and K would stay the same.

2) Which of the following is true regarding the effect of acatalyst on chemical equilibrium?

a.	Only the forward rate increases so the quantity of productsincreases.
b.	Only the forward rate increases but the quantity of productsremains the same.
c.	Both the forward and reverse rates increase and the quantity ofproducts increases.
d.	Both the forward and reverse rates increase but the quantity ofproducts is unchanged.
e.	The effect varies depending on whether the reaction isendothermic or exothermic.

3) The equilibrium constant for a given reaction __________

a.	does not change with temperature.
b.	always increases with temperature.
c.	always decreases with temperature.
d.	increases with temperature for exothermic reactions only.
e.	increases with temperature for endothermic reactions only,

Fill in the blanks

1) Chemical equilibrium arises from the __________ of chemicalreactions and is defined when the __________ of the forwardreaction is equal to the __________ of the reverse reaction.

2) Students often write expressions for the equilibrium constantK_c and reaction quotient Q_cin exactly the same way. To avoid confusion, you must rememberthatK_c uses concentrations under __________conditions while Q_c uses concentrations under__________ conditions.

3) If Q for a reaction is greater than K, thereaction will be __________. If Q for a reaction is lessthan K, the reaction will be __________. If Q fora reaction is equal to K, the reaction will be__________.

4) How and why are the expressions for homogeneous equilibriumconstants different from the expressions for heterogeneousequilibrium constants?

1) If the temperature of an endothermic reaction at equilibriumcould be increased instantaneously, what would be the instantaneouseffect on Q and K before equilibrium was againachieved?

a.	Q would increase and K would stay thesame.
b.	Q would decrease and K would stay thesame.
c.	Q would stay the same and K wouldincrease.
d.	Q would stay the same and K woulddecrease.
e.	Both Q and K would stay the same.

2) Which of the following is true regarding the effect of acatalyst on chemical equilibrium?

a.	Only the forward rate increases so the quantity of productsincreases.
b.	Only the forward rate increases but the quantity of productsremains the same.
c.	Both the forward and reverse rates increase and the quantity ofproducts increases.
d.	Both the forward and reverse rates increase but the quantity ofproducts is unchanged.
e.	The effect varies depending on whether the reaction isendothermic or exothermic.

3) The equilibrium constant for a given reaction __________

a.	does not change with temperature.
b.	always increases with temperature.
c.	always decreases with temperature.
d.	increases with temperature for exothermic reactions only.
e.	increases with temperature for endothermic reactions only,

Fill in the blanks

1) Chemical equilibrium arises from the __________ of chemicalreactions and is defined when the __________ of the forwardreaction is equal to the __________ of the reverse reaction.

2) Students often write expressions for the equilibrium constantK_c and reaction quotient Q_cin exactly the same way. To avoid confusion, you must remember thatK_c uses concentrations under __________conditions while Q_c uses concentrations under__________ conditions.

3) If Q for areaction is greater than K, thereaction will be __________. If Q for areaction is less than K, thereaction will be __________. If Q for areaction is equal to K, thereaction will be __________.

4) How and why are the expressions for homogeneous equilibriumconstants different from the expressions for heterogeneousequilibrium constants?

Listed in the table are forward and reverse rate constants for the reaction: 2NO(g)
kf
ï¿½ï¿½
kr
ï¿½ï¿½ N2(g) + O2(g)
Temperature (K) Kf (M-1s-1) Kr (M-1s-1)
1400 0.29 1.1Ã10-6
1500 1.3 1.4Ã10-5
(a) Determine a value for the equilibrium constant at each temperature {4 points}
(b) Is this reaction exothermic or endothermic? {1 points}

Ammonia reacts with carbon dioxide to form a solid, NH4CO2NH2 according to the following reaction:
2NH3(g) + CO2(g) â NH4CO2NH2(s)
Where Kp = 0,614 (atm-3) at 298 K. If equilibrium is established at 298 K by starting with pure solid, what is the partial
pressures of NH3 and CO2 at equilibrium? What is the total pressure at equilibrium?

Chemistry 1027A/B Lecture Notes - Gas Constant, Inert Gas, Equilibrium Constant

Document Summary

Get access

Related Documents

Chemistry 1027A/B Study Guide - Final Guide: Reaction Mechanism, Half-Life, Nernst Equation

Chemistry 1027A/B Study Guide - Coordinate Covalent Bond, Ionic Compound, Equilibrium Constant

Chemistry 1027A/B Chapter Notes - Chapter 1.1: Endothermic Process, Gibbs Free Energy, Reaction Quotient

Related Questions