Balance the following redox reaction in acidic solution: H+(aq)+Zn(s)→H2(g)+Zn2+(aq)

1 answer:

5 0

2H⁺(aq) + Zn(s) ----> H2(g) + Zn²⁺(aq)

2H⁺(aq) +2e⁻ ----->H2(g) reduction
Zn(s) ------>Zn²⁺ +2e⁻ oxidation
2H⁺(aq) + Zn(s) -----> H2(g) + Zn²⁺

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Answer:

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Explanation:

Carbon-14 is radioactive and it follows the first-order kinetics for a radioactive decay. The first-order kinetics may be described by the following integrated rate law:

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Here:

$[A]_t$ is the mass, moles, molarity or percentage of the material left at some time of interest t;

$[A]_o$ is the mass, moles, molarity or percentage of the material initially, we know that initially we expect to have 100 % of carbon-14 before it starts to decay;

$k = \frac{ln(2)}{T_{\frac{1}{2}}}$ is the rate constant;

$t$ is time.

The equation becomes:

$ln(\frac{[A]_t}{[A]_o})=-\frac{ln(2)}{T_{\frac{1}{2}}}t$

Given:

$\frac{[A]_t}{[A]_o} = \frac{40.0 %}{100.0 %}$

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Solve for time:

$t = -\frac{ln(\frac{[A]_t}{[A]_o})\cdot T_{\frac{1}{2}}}{ln(2)}$

In this case:

$t = -\frac{ln(\frac{40.0\%}{100.0\%})\cdot 5770 y}{ln(2)}$

$t = 7628 y$

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Why is the value listed for atomic mass for each element on the periodic table not a whole number?

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A. it is an average

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Actual question from source:-

A 3.96x10-4 M solution of compound A exhibited an absorbance of 0.624 at 238 nm in a 1.000 cm cuvette. A blank had an absorbance of 0.029. The absorbance of an unknown solution of compound A was 0.375. Find the concentration of A in the unknown.

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