Metal Reactivity and Corrosion Protection
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Using the following equations, which represent spontaneous reactions: (Exam 4 L1 Ch5)
$$Y_{(s)} + Z^{2+}_{(aq)} \rightarrow Y^{2+}_{(aq)} + Z_{(s)}$$
$$X^{2+}_{(aq)} + Y_{(s)} \rightarrow X_{(s)} + Y^{2+}_{(aq)}$$
Which of the following statements is probable to be true due to insufficient information?
a) plating element Y with element X represents anodic protection.
b) plating element X with element Y represents anodic protection.
c) plating element Z with element X represents cathodic protection.
d) plating element Y with element Z represents cathodic protection.
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In this problem, we are given two spontaneous redox reactions and asked to determine which statement regarding corrosion protection is true based on the relative reactivity of elements X, Y, and Z.
Electrochemistry and Corrosion Protection
Let's list the spontaneous reactions provided to deduce the relative activity of the metals. Reaction one shows solid Y reacting with Z two plus ions to give Y two plus ions and solid Z.
Given Reactions (Spontaneous)
Since this reaction is spontaneous, metal Y is more reactive than metal Z. It means Y has a higher tendency to oxidize than Z.
Now let's look at the second reaction. X two plus ions react with solid Y to produce solid X and Y two plus ions.
Because this is also spontaneous, solid Y is more reactive than solid X. Y oxidizes while X ions are reduced.
Now we need to compare X and Z. The first reaction tells us Y is better than Z at reducing, and the second tells us Y is better than X at reducing. However, we don't have a direct reaction between X and Z to determine their relative order.
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