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Veronika [31]
3 years ago
13

What is the empirical formula of the compound that is 25.3% magnesium and 74.7% chlorine

Chemistry
1 answer:
Margarita [4]3 years ago
4 0

Answer: MgCl_2

Explanation:

25.3% Mg

74.7% Cl

First step: change % to g

25.3g Mg

74.7g Cl

Second step: calculate g/mol of each compound. You can do this by using the atomic mass.

25.3gMg(\frac{1mol}{24.30g})=1.04mol

74.7gCl(\frac{1mol}{35.45g} )=2.11mol

Third step: determine the lowest number and divide everything by it. Of the result, extract whole number only.

Mg=\frac{1.04}{1.04} =1

Cl=\frac{2.11}{1.04}=2

Fourth step: Write each compound with their respective number below.

This empirical formula should be: MgCl_2

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Partial pressure of nitrogen gas.p_{N_2}=53 atm=53\times 760 torr= 40,280 torr (1atm = 760 torr)

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Answer :

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Explanation :

First we have to calculate the concentration of H^+ before any titrant is added to our starting material.

As we are given:

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As we know that the HBr is a strong acid that dissociates complete to give hydrogen ion H^+ and bromide ion Br^-.

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