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inysia [295]
3 years ago
9

A chloride of this element is 67.2% chlorine by mass. In a 100 g sample how many moles of chlorine are there? (This info will be

used to determine the empirical formula. Because the accuracy of the result in the last question for this set of questions depends on the accuracy of this answer, use the atomic mass of Cl accurate to 4 SIG. FIG.).
Chemistry
1 answer:
Ann [662]3 years ago
4 0

Answer:

1.896 mol Cl

Explanation:

  • Because the chloride is 67.2% chlorine by mass, i<u>n a 100 g sample of this compound, we would have 67.2 g of chlorine.</u>

With that information then we can calculate <u>the moles of chlorine</u> present in 67.2 g, using its atomic mass (accurate to 4 sig. fig. as the exercise asked):

67.2 g Cl ÷ 35.45 g/mol = 1.896 mol Cl

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Explanation:

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In Na2O, what is the oxidation state of oxygen? In Na2O oxidation state of Na is 1+
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3 years ago
Substances like neon , which is a gas at room temperature and pressure, can often be liquified or solidified only at very low te
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Answer:

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In order to solve this above question, there is is need to make use of the following equation. The main idea here is to convert degree celsius to Kelvin. Hence,

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3 years ago
What is the empirical formula of a compound containing 90 grams carbon, 11 grams hydrogen, and 35 grams nitrogen?
Anvisha [2.4K]

Answer:

= C3H4N

Explanation:

We are given; 90 grams carbon, 11 grams hydrogen, and 35 grams nitrogen.

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Carbon = 90g/12 g/mol

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Hydrogen = 11 g/ 1 g/mol

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Nitrogen = 35 g/ 14 g/mol

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= 7.5/2.5 : 11/2.5 : 2.5 /2.5

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= 3 : 4 : 1

Therefore;

The empirical formula will be; C3H4N

6 0
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