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polet [3.4K]
3 years ago
7

PLEASE HELP 16. (4 points) Sodium reacts with oxygen to produce sodium oxide as described by the balanced equation below. If 54.

1g of sodium reacts with excess oxygen gas to produce 61.8g of sodium oxide, what is the percent yield? Show all work. (hint: be sure to calculate theoretical yield first)
4Na + O2 --> 2Na2O
Chemistry
1 answer:
never [62]3 years ago
4 0
Percent yield of the equation at above condidtions will be 42.4%
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How many half-lives are required for the concentration of reactant to decrease to 1.56% of its original value?4247.56.56
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Answer:

6 half-lives are required for the concentration of reactant to decrease to 1.56% of its original value.

Explanation:

Using integrated rate law for first order kinetics as:

[A_t]=[A_0]e^{-kt}

Where,

[A_t] is the concentration at time t

[A_0] is the initial concentration

Given:

Concentration is decreased to 1.56 % which means that 0.0156 of [A_0] is decomposed. So,

\frac {[A_t]}{[A_0]} = 0.0156

Thus,

\frac {[A_t]}{[A_0]}=e^{-k\times t}

0.0156=e^{-k\times t}

kt = 4.1604

The expression for the half life is:-

Half life = 15.0 hours

t_{1/2}=\frac {ln\ 2}{k}

Where, k is rate constant

So,  

k=\frac {ln\ 2}{t_{1/2}}

\frac{4.1604}{t}=\frac {ln\ 2}{t_{1/2}}

t = 6\times t_{1/2}

<u>6 half-lives are required for the concentration of reactant to decrease to 1.56% of its original value.</u>

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