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Amiraneli [1.4K]
3 years ago
10

Using the Hoffman apparatus for electrolysis, a chemist decomposes 2.3 moles of water into its gaseous elements. How many grams

of hydrogen gas should get (theoretical yield)? The chemist collected 2.0 moles hydrogen gas. What is his percent yield?
Chemistry
1 answer:
solong [7]3 years ago
7 0

Answer:

2.318032g

Explanation:

-The electrolysis equation of water is written as below:

2H_2O_{(l)}->2H_2_{(g)}+O_2_{(g)}

-The mole ratio of Water to the hydrogen formed is 1:1, therefore 2.3 moles of hydrogen gas is produced.

-Hydrogen's molar mass is 1.00784 grams:

Mass=moles\times molar \ mass\\\\\=2.3\times 1.00784\\\\=2.318032\ g

Hence, 2.318032 grams of hydrogen is produced.

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Calculate the concentration of all ions present in each of the following solutions of strong electrolytes. a. 0.100 mole of Ca(N
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Answer:

[Ca²⁺] = 1M

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Explanation:

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The moles of Ca²⁺ can be found using the molar relationship between Ca(NO₃)₂ and Ca²⁺

(0.100mol Ca(NO₃)₂) (Ca²⁺ /Ca(NO₃)₂) = 0.100 mol Ca²⁺

The concentration of Ca²⁺  is then:

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Similarly, moles of NO₃⁻ can be found using the molar relationship between Ca(NO₃)₂ and NO₃⁻:

(0.100mol Ca(NO₃)₂) (2NO₃⁻/Ca(NO₃)₂) = 0.200 mol NO₃⁻

The concentration of NO₃⁻ is then:

[NO₃⁻] = (0.200mol)/(100.0mL) x (1000ml)/(1L) = 2M

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