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2 years ago

The elemental composition of a compound is determined to be 39.5% oxygen, 32.1% chromium and 28.4% sodium by weight.

Chemistry

1 answer:

maksim [4K]2 years ago

3 0

Answer:

Explanation:

To calculate percent composition, we divide the experimentally derived mass of each element by the overall mass of the compound, and then convert to a percentage:

%C=

12.04g compound

7.34g C

×100%=61.0%

%H=

12.04g compound

1.85g H

×100%=15.4%

%N=

12.04g compound

2.85g N

×100%=23.7%

The analysis results indicate that the compound is 61.0% C, 15.4% H, and 23.7% N by mass.

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2 years ago

The balanced equation for combustion in an acetylene torch is shown below: 2C2H2 + 5O2 → 4CO2 + 2H2O The acetylene tank contains

andriy [413]

Answer: 67.2 moles

Explanation: $2C_2H5+5O_2\rightarrow 4CO_2+2H_2O$

According to the given balanced equation, 2 moles of acetylene $C_2H_2$ combine with 5 moles of oxygen $O_2$ to produce 4 moles of carbon dioxide $CO_2$ .

Thus if 2 moles of acetylene $C_2H_2$ combine with = 5 moles of oxygen $O_2$

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But as only 84 moles of oxygen are available, acetylene is not a limiting reagent.

5 moles of oxygen $O_2$ reacts with = 2 moles of acetylene $C_2H_2$

84 moles of oxygen $O_2$ reacts with= $\frac{2}{5}\times {84}=33.6$ moles of acetylene $C_2H_2$

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2 moles of acetylene $C_2H_2$ produce= 4 moles of carbon dioxide $CO_2$ .

33.6 moles of acetylene $C_2H_2$ produce= $\frac{4}{2}\times {33.6}=67.2$ moles of of carbon dioxide $CO_2$ .

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3 years ago

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