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3 years ago

If the density of an ideal gas at stp if found to be 0.0902 g/l, what is its molar mass?

Chemistry

2 answers:

alina1380 [7]3 years ago

6 0

<u>Answer:</u> The molar mass of the gas is 2.02 grams.

<u>Explanation:</u>

We are given:

Density of gas = 0.0902 g/L

At STP conditions:

1 mole of gas occupies 22.4 L of volume

And 1 mole of a substance is known as the molecular mass or molar mass of that substance.

To calculate the mass of gas, we use the equation:

$\text{Density of gas}=\frac{\text{Mass of gas}}{\text{Volume of gas}}$

Putting values in above equation, we get:

$0.0902g/L=\frac{\text{Mass of gas}}{22.4L}\\\\\text{Mass of gas}=2.02g$

Hence, the molar mass of the gas is 2.02 grams.

lisabon 2012 [21]3 years ago

4 0

P=0.0902 g/l
v=22.4 l/mol (stp)

M=vp

M=22.4 l/mol * 0.0902 g/l=2.020 g/mol

M=2.020 g/mol

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What is the empirical formula for a compound that contains 10.89% magnesium 31.77% chloride and 57.34% oxygen

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Answer: $Mg_{1}Cl_{2}O_{8}$

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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.

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Step 1 : convert given masses into moles.

Moles of Mg= $\frac {\text{ given mass of Mg}}{\text{ molar mass of Mg}}= \frac {10.89g}{24g/mole}=0.45moles$

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Moles of O = $\frac {\text{ given mass of O}}{\text{ molar mass of O}}=\frac {57.34g}{16g/mole}=3.58moles$

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

For Mg = $\frac {0.45}{0.45}=1$

For Cl = $\frac {0.89}{0.45}=2$

For O= $\frac {3.58}{0.45}=8$

The ratio of Mg :Cl : O= 1 : 2 : 8

Hence the empirical formula is $Mg_{1}Cl_{2}O_{8}$

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Answer: 824.6 g of NaCl are produced from 500.0 g of chlorine.

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$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$ $\text{Moles of} Cl_2=\frac{500.00g}{71g/mol}=7.04moles$

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