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NeX [460]
3 years ago
8

What volume of hydrogen iodide is produced when 118 liters of hydrogen gas react according to the following reaction? (All gases

are at the same temperature and pressure.) hydrogen(g) + iodine(s) hydrogen iodide(g) liters hydrogen iodide
Chemistry
1 answer:
Nadya [2.5K]3 years ago
4 0

Answer:

V_{HI}=236LHI

Explanation:

Hello,

In this case, for the given balanced chemical reaction:

H_2(g)+I_2(g)\rightarrow 2HI(g)

Thus, since hydrogen and hydrogen iodide are in a 1:2 mole ratio, we can easily compute the yielded volume as shown below:

V_{HI}=118LH_2*\frac{2molHI}{1molH_2} \\\\V_{HI}=236LHI

Thus, is possible, due to the Avogadro's law which allows to relate moles and volume by a directly proportional relationship.

Regards.

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2 years ago
A sample of 53.0 of carbon dioxide was obtained by heating 1.31 g of calcium carbont. What is the percent yield for this reactio
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Answer:

92.04%

Explanation:

Given:

Mass of CO₂ obtained = 53.0 grams

Mass of calcium carbonate heated = 1.31 grams

Now,

the molar mass of the calcium carbonate = 100.08 grams

The number of moles heated in the problem = Mass  / Molar mass

= (1.31 grams) / (100.08 grams/moles)

= 0.013088 moles

now,

1 mol of calcium carbonate yields 1 mol of CO₂

thus,

0.013088 moles of calcium carbonate will yield = 0.013088 mol of CO₂

now,

Theoretical mass of 0.013088 moles of CO₂ will be

= Number of moles × Molar mass of CO₂

= 0.013088 × 44 = 0.5758  grams

Thus, the percent yield for this reaction = \frac{\textup{Actual yield}}{\textup{Theoretical yield}}\times100

or

the percent yield for this reaction = \frac{0.53}{0.5758}\times100

or

the percent yield for this reaction = 92.04%

6 0
3 years ago
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