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dusya [7]
3 years ago
10

What is the density in g/L of gas with a molar mass of 2.016 g/mol at 4.77 atm and 118k?

Chemistry
2 answers:
sladkih [1.3K]3 years ago
7 0

Answer:

0.9926 g/L is the density of gas.

Explanation:

Molar mass of gas = M = 2.016 g/mol

Mass of  gas = m

Density of the gas = d =\frac{Mass}{Volume}=\frac{m}{V}...(1)

Pressure of the gas = 4.77 atm

Temperature of the gas = T = 118 K

PV=nRT=\frac{m}{M}RT

P=\frac{m}{V\times M}RT

\frac{P\times M}{RT}=d..(From (1))

d=\frac{4.77 atm\times 2.016 g/mol}{0.0821 atm l/mol K\times 118 K}

d = 0.9926 g/L

0.9926 g/L is the density of gas.

kotegsom [21]3 years ago
5 0

n / V = P / RT = (4.77 atm) / ((0.08205746 L atm/K mol) x (118 K)) = 0.4926 mol/L

(2.016 g/mol) x (0.4926 mol/L) = 0.993 g/L

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How would you prepare 500 mL of 0.360 M solution of CaCl2 from<br> solid CaCl2?
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We need to measure 20.0 grams of CaCl₂ to prepare 500 mL of 0.360 M solution.

First, we need to determine the required moles of CaCl₂. We have 500 mL (0.500 L) of a 0.360 M solution (0.360 moles of CaCl₂ per liter of solution).

0.500 L \times \frac{0.360mol}{L} = 0.180 mol

Then, we will convert 0.180 moles to grams using the molar mass of CaCl₂ (110.98 g/mol).

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To prepare the solution, we weigh 20.0 g of CaCl₂ and add it to a beaker with enough distilled water to dissolve it. We stir it, heat it if necessary, and when we have a solution, we transfer it to a 500 mL flask and complete it to the mark with distilled water.

We need to measure 20.0 grams of CaCl₂ to prepare 500 mL of 0.360 M solution.

You can learn more about solutions here: brainly.com/question/2412491

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Answer:

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