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den301095 [7]
3 years ago
6

A 3.8 g sample of sodium hydrogen carbonate is added to a solution of acetic acid weighing 10.8 g. The two substances react, rel

easing carbon dioxide gas to the atmosphere. After the reaction, the contents of the reaction vessel weigh 11.6 g. What is the mass of carbon dioxide released during the reaction
Chemistry
1 answer:
UkoKoshka [18]3 years ago
8 0

Answer:

3.0 g

Explanation:

The <em>total mass </em>at the beginning of the reaction is:

  • 3.8 g + 10.8 g = 14.6 g

Following the law of conservation of mass, this same mass has to be present once the reaction is complete. This means that the mass diference between <em>the contents of the reaction vessel after the reaction and the mass at the beginning of the reaction</em> is the mass of released carbon dioxide:

  • 14.6 g - 11.6 g = 3.0 g
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To determine the empirical formula of the compound given, we need to determine the ratio of each element in the compound. To do that we assume to have 100 grams sample of the compound with the given composition. Then, we calculate for the number of moles of each element. We do as follows:<span>
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C       56.79        4.73
H       6.56          6.50
O       28.37        1.77
N      8.28           0.59

Dividing the number of moles of each element with the smallest value, we will have the empirical formula:

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C       4.73     / 0.59       8
H       6.50     / 0.59      11
O       1.77     / 0.59       3
N        0.59    / 0.59       1<span>
</span><span>
The empirical formula would be C8H11O3N.</span>
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