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pogonyaev
2 years ago
5

Upon decomposition, one sample of magnesium fluoride produced 1.65 kg of magnesium and 2.56 kg of fluorine. A second sample prod

uced 1.32 kg of magnesium. Part A How much fluorine (in grams) did the second sample produce?
Chemistry
1 answer:
aleksley [76]2 years ago
7 0

Answer : The mass of fluorine in second sample produces, 2.048 grams

Law of definite proportion states that in a chemical compound, the components of the element are in fixed ratio.

The given chemical compound is magnesium fluoride. In the magnesium fluoride the components of the element magnesium and fluorine are in fixed ratio that is, 1 : 1

\frac{M_{Mg}}{M_{F}}=\frac{m_{Mg}}{_{F}}

M_{Mg} = mass of magnesium in sample 1 = 1.65 g

M_{F} = mass of fluorine in sample 1 = 2.56 g

m_{Mg} = mass of magnesium in sample 2 = 1.32 g

m_{F} = mass of fluorine in sample 2 = x

Now put all the give values in the above relation, we get

\frac{1.65g}{2.56g}=\frac{1.32g}{x}

x=2.048g

Therefore, the mass of fluorine in second sample produces, 2.048 grams

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This problem could be solved easily using the Henderson-Hasselbach equation used for preparing buffer solutions. The equation is written below:

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Moles of salt = 1 mol/L * 25 mL * 1 L/1000 mL = 0.025 moles salt
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4 0
2 years ago
Which state of matter are particles packed tightly together and fix positions
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3 years ago
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Average atomic mass of chlorine is 35.48 amu.

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   From the balanced chemical equation;

          2 moles of AgNO₃  will produce 1 mole of Ag₂CrO₄

          4.85 moles of AgNO₃  will produce \frac{4.85}{2}   = 2.43moles of Ag₂CrO₄

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