MC_Chem1B_Sp098_LabQuiz1

Multiple Choice
Identify the choice that best completes the statement or answers the question.

In  reactions involving the iodination of acetone, the following volumes were used to make up the reaction mixtures:
MIXTURE 1: 10 mL of 4M acetone + 10 mL of 1.0 M HCl +10 mL 0.005 M I2 + 20 mL H2O
MIXTURE 2: 20 mL of 4M acetone + 10 mL of 1.0 M HCl +10 mL 0.005 M I2 + 10 mL H2O
MIXTURE 3: 20 mL of 4M acetone + 10 mL of 1.0 M HCl +20 mL 0.005 M I2

____	1.	What is the initial molarity of acetone in the rxn. MIXTURE 1:

a.	0.2	b.	0.4	c.	0.04	d.	0.08	e.	0.8	

____	2.	What is the initial molarity of HCl in rxn MIXTURE 1?

a.	0.01	b.	0.05	c.	0.1	d.	0.2	e.	None of these	

____	3.	What is the initial molarity of I2 in rxn MIXTURE 1?

a.	0.02	b.	0.001	c.	0.0005	d.	0.10	e.	None of these 	

____	4.	If it took 250 second for the iodine to disappear from the reaction MIXTURE 1, What was the rate of the reaction in MIXTURE 1?

a.	2.2 x 10-5	b.	4.2 x 10-5	c.	4.2 x 10-6	d.	1.2 x 10-6	e.	1.2 x 10-4	

____	5.	If it took 120 second for the iodine to disappear from the reaction MIXTURE 2, What was the rate of the reaction in MIXTURE 2?

a.	2.3 x 10-4	b.	1.3 x 10-6	c.	8.3 x 10-3	d.	4.0 x 10-6	e.	8.3 x 10-6	

____	6.	How many minutes will it take for the iodine to disappear from the reaction MIXTURE 3?

a.	40.0	b.	250	c.	120	d.	4.00	e.	240	

____	7.	If you mix 10.00 mL of 2.00 x 10-3 M Fe(NO3)3 with 10.00 mL of 2.00 x 10-3 M NaSCN and then after equilibration, the concentration of FeSCN2+ is 1.40 x 10-4 M, then calculate the number of moles of  Fe3+ ion in the equlibrium mixture: Fe3+(aq) + SCN-(aq) <=> FeSCN2+(aq)
a.	8.6x10-5	b.	8.6x10-4	c.	1.3x10-6	d.	8.6x10-6	e.	1.72x10-5	

____	8.	If you mix 10.00 mL of 2.00 x 10-3 M Fe(NO3)3 with 10.00 mL of 2.00 x 10-3 M NaSCN and then after equilibration, the concentration of FeSCN2+ is 1.40 x 10-4 M, then calculate the number of moles of  SCN-  ion in the equlibrium mixture: Fe3+(aq) + SCN-(aq) <=> FeSCN2+(aq)
a.	9.6x10-5	b.	8.6x10-6	c.	1.72x10-5	d.	1.72x10-4	e.	1.72x10-6	

____	9.	If you mix 10.00 mL of 2.00 x 10-3 M Fe(NO3)3 with 10.00 mL of 2.00 x 10-3 M NaSCN and then after equilibration, the concentration of FeSCN2+ is 1.40 x 10-4 M, then calculate [SCN- ] in the equlibrium mixture: Fe3+(aq) + SCN-(aq) <=> FeSCN2+(aq)
a.	2.6x10-5	b.	8.6x10-9	c.	5.6x10-6	d.	8.6x10-4	e.	1.4x10-3	

____	10.	If you mix 10.00 mL of 2.00 x 10-3 M Fe(NO3)3 with 10.00 mL of 2.00 x 10-3 M NaSCN and then after equilibration, the concentration of FeSCN2+ is 1.40 x 10-4 M, then calculate [Fe3+ ] in the equlibrium mixture: Fe3+(aq) + SCN-(aq) <=> FeSCN2+(aq)
a.	1.6X10-4	b.	8.6X10-6	c.	2.6X10-9	d.	8.6X104	e.	8.6X10-4	

____	11.	If you mix 10.00 mL of 2.00 x 10-3 M Fe(NO3)3 with 10.00 mL of 2.00 x 10-3 M NaSCN and then after equilibration, the concentration of FeSCN2+ is 1.40 x 10-4 M, then calculate Kc of the equlibrium reaction: Fe3+(aq) + SCN-(aq) <=> FeSCN2+(aq)
a.	921	b.	543	c.	296	d.	189	e.	111	

____	12.	If you mix 10.00 mL of 2.00 x 10-3 M Fe(NO3)3 with 10.00 mL of 2.00 x 10-3 M NaSCN and then after equilibration, the concentration of Fe(SCN)2+ is 7.00 x 10-5 M, then calculate the Kc of the equlibrium reaction: Fe3+(aq) + 2 SCN-(aq) <=> Fe(SCN)2+(aq)
a.	9.35x102	b.	1.35x104	c.	1.02x105	d.	1.35x10-6	e.	9.35x106	

____	13.	The reaction of NO and O2 produces NO2.

2 NO(g) + O2(g) ® 2 NO2(g)

The reaction is second-order with respect to NO(g) and first-order with respect to O2(g). At a given temperature, the rate constant, k, equals 6.1 ´ 103 M-2s-1. What is the rate of reaction when the initial concentrations of NO and O2 are 0.020 M and 0.015 M, respectively?
a.	9.8 ´ 10-10 M/s	
b.	0.027 M/s	
c.	0.037 M/s	
d.	1.0 M/s	
e.	1.8 M/s	

____	14.	For a given reaction, the rate constant doubles when the temperature is increased from 37 °C to 51 °C. What is the activation energy for this reaction? (R = 8.314 J/K·mol)
a.	18 kJ/mol	
b.	41 kJ/mol	
c.	59 kJ/mol	
d.	86 kJ/mol	
e.	780 kJ/mol	

____	15.	Write a balanced chemical equation which corresponds to the following equilibrium constant expression.

Kp = 

a.	1/2 N2(g) + 3/2 H2(g) f NH3(g)	
b.	N2(g) + 3 H2(g) f 2 NH3(g)	
c.	2 NH3(g) f N2(g) + 3 H2(g)	
d.	NH3(g) f 1/2 N2(g) + 3/2 H2(g)	
e.	2 N2(g) + 6 H2(g) f 4 NH3(g)	

____	16.	Excess Ca(IO3)2(s) is placed in 1.5 L of water. At equilibrium, the solution contains 0.011 M IO3-(aq). What is the equilibrium constant for the reaction below?

Ca(IO3)2(s) f Ca2+(aq) + 2 IO3-(aq)

a.	3.3 ´ 10-7	
b.	6.7 ´ 10-7	
c.	1.3 ´ 10-6	
d.	5.3 ´ 10-6	
e.	6.1 ´ 10-5	

MC_Chem1B_Sp098_LabQuiz1
Answer Section

MULTIPLE CHOICE

	1.	ANS:	E	PTS:	1

	2.	ANS:	D	PTS:	1

	3.	ANS:	B	PTS:	1

	4.	ANS:	C	PTS:	1

	5.	ANS:	E	PTS:	1

	6.	ANS:	D	PTS:	1

	7.	ANS:	E	PTS:	1

	8.	ANS:	C	PTS:	1

	9.	ANS:	D	PTS:	1

	10.	ANS:	E	PTS:	1

	11.	ANS:	D	PTS:	1

	12.	ANS:	C	PTS:	1

	13.	ANS:	C	PTS:	1	OBJ:	15.3 Effect of Concentration on Reaction Rate

	14.	ANS:	B	PTS:	1	OBJ:	15.5 A Microscopic View of Reaction Rates

	15.	ANS:	A	PTS:	1	OBJ:	16.2 The Equilibrium Constant and the Reaction Quotient

	16.	ANS:	B	PTS:	1	OBJ:	16.3 Determining an Equilibrium Constant