Self Assessment A


1	When the following redox reaction is balanced, the coefficient for S is _____. HNO₃ + H₂S ----> NO + S + H₂O
		A)	1
		B)	3
		C)	4
		D)	8
		E)	10


2	Which is true about the following balanced redox reaction: 3 CuO(s) + 2 NH₃(aq) ----> N₂(g) + 3 H₂O(l) + 3 Cu(s)?
		A)	CuO is the oxidizing agent and Cu is oxidized.
		B)	CuO is the reducing agent and Cu is reduced.
		C)	CuO is the oxidizing agent and Cu is reduced.
		D)	CuO is the reducing agent and Cu is oxidized.


3	Which component of the following cell is the cathode? K\|L\|M\|N
		A)	K
		B)	L
		C)	M
		D)	N


4	A voltaic cell is prepared using zinc and iron. Its cell notation is as follows: Zn\|Zn²⁺(1 M)\|Fe²⁺(1 M)\|Fe³⁺(1M)\|Pt. Which of the following reactions occurs at the cathode?
		A)	Fe³⁺ + e^- ----> Fe²⁺
		B)	Fe²⁺ ----> Fe³⁺ + e^-
		C)	Zn ----> Zn²⁺ + 2 e^-
		D)	Zn²⁺ + 2e^- ----> Zn


5	A cell can be prepared from zinc and iron. What is the E^o_cell for the cell that forms from the following half reactions? Fe³⁺ + e^- ----> Fe²⁺, E^o = 0.77 V; Zn²⁺ + 2e^- ----> Zn, E^o = -0.76 V
		A)	-1.53 V
		B)	-0.01 V
		C)	0.78 V
		D)	0.01 V
		E)	1.53 V


6	Examine the following half-reactions and select the strongest oxidizing agent among the substances: Sr²⁺ + 2 e^- ----> Sr, E^o = -2.89 V; Cr²⁺ + 2 e^- ----> Cr, E^o = -0.913 V; Fe²⁺ + 2 e^- ----> Fe, E^o = -0.447 V; Co²⁺ + 2 e^- ----> Co, E^o = -0.28 V.
		A)	Cr²⁺
		B)	Sr²⁺
		C)	Co²⁺
		D)	Fe²⁺


7	Calculate the equilibrium constant for the reaction: 2 Cr + 3 Pb²⁺ ----> 3 Pb + 2 Cr³⁺ at 25 ^oC. E^o_cell = 0.61 V.
		A)	4 x 10²⁰
		B)	8 x 10³⁰
		C)	9 x 10⁴⁵
		D)	3 x 10⁵¹
		E)	7 x 10⁶¹


8	The equilibrium constant for the reaction of Ni²⁺ with Cd is 1.17 x 10⁵. Calculate (G for the reaction at 25 ^oC.
		A)	-12.6 kJ
		B)	-28.9 kJ
		C)	2.43 kJ
		D)	28.9 kJ
		E)	12.6 kJ


9	What is the potential of the following cell: Cu\|Cu²⁺ (0.001 M)\|Cu²⁺(1 M)\|Cu? [Cu²⁺ + 2e^- ----> Cu E^o = 0.342 V]
		A)	-0.253 V
		B)	0.253 V
		C)	-0.0887 V
		D)	0.0887 V
		E)	None of the above.


10	What mass of copper can be deposited by the passage of 12.0 A for 25.0 min through a solution of copper(II) sulfate. [1 C = 1 A·s; F = 96,500 C]
		A)	5.93 g
		B)	3.95 g
		C)	1.97 g
		D)	11.85 g
		E)	29.6 g

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