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denis-greek [22]
3 years ago
11

combustion analysis of an unknown compound provides the following data: 73.5 grams carbon (C), 4.20 grams hydrogen (H) and 72.3

grams chlorine (Cl). What is the percent composition of each element in this compound?
Chemistry
1 answer:
Alex17521 [72]3 years ago
4 0
M(C)=73.5 g
m(H)=4.20 g
m(Cl)=72.3 g

mass of compound
m=m(C)+m(H)+m(Cl)

m=73.5+4.20+72.3=150 g

w(H)=100m(H)/m
w(H)=100*4.20/150=2.8%

w(Cl)=100m(Cl)/m
w(Cl)=100*72.3/150=48.2%

w(C)=100-w(H)-w(Cl)
w(C)=100-2.8-48.2=49.0%
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What is the empirical formula of a compound that contains 49.4% K, 20.3% S, and 30.3% by mass? A) KSO3 B) K2SO3 C) KSO2 D) KSO E
yulyashka [42]

Answer: K_2SO_3.

Explanation:

If percentage are given then we are taking total mass is 100 grams.

So, the mass of each element is equal to the percentage given.

Mass of K = 49.4 g

Mass of S = 20.3 g

Mass of O = 30.3 g

Step 1 : convert given masses into moles.

Moles of K=\frac{\text{ given mass of K}}{\text{ molar mass of K}}= \frac{49.4g}{40g/mole}=1.23moles

Moles of S= \frac{\text{ given mass of S}}{\text{ molar mass of S}}= \frac{20.3g}{32g/mole}=0.63moles[/tex]

Moles of O = \frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{30.3g}{16g/mole}=1.89moles[/tex]

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For K = \frac{1.23}{0.63}=2

For S =\frac{0.63}{0.63}=1

For O =\frac{1.89}{0.63}=3

The ratio of K: S:O = 2: 1: 3

Hence the empirical formula is K_2SO_3.

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