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Pavlova-9 [17]
2 years ago
10

A sample of an unknown compound is vaporized at . The gas produced has a volume of at a pressure of , and it weighs . Assuming t

he gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Be sure your answer has the correct number of significant digits.
Chemistry
1 answer:
Likurg_2 [28]2 years ago
8 0

Answer:

The answer is "34 \ \frac{g}{mol}"

Explanation:

Please find the complete question in the attached file.

Formula:

\to PV = nRT\\\\n = \frac{mass}{MW} \\\\PV = \frac{mRT}{MW}\\\\MW = \frac{mRT}{(PV)}\\\\MW = \frac{(0.941)(0.082)(150+273)}{(1 \times 0.96)}

        = \frac{(0.941)(0.082)(423)}{(0.96)} \\\\= \frac{32.639526}{(0.96)} \\\\= 33.9995062\ \ \ or \ \ \ 34 \ \frac{g}{mol}

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3 years ago
A 3.0-L sample of helium was placed in container fitted with a porous membrane. Half of the helium effused through the membrane
zhenek [66]

Explanation:

It is known that rate of effusion of gases are inversely proportional to the square root of their molar masses.

And, half of the helium (1.5 L) effused in 24 hour. So, the rate of effusion of He gas is calculated as follows.

          \frac{1.5 L}{24 hr}

            = 0.0625 L/hr

As, molar mass of He is 4 g/mol  and molar mass of O_{2} is 32 g/ mol.

Now,

   \frac{\text{Rate of He}}{\text{Rate of Oxygen}} = \sqrt{\frac{32}{4}

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or, rate of O_{2} = \frac{\text{Rate of He}}{2.83}

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This means that 0.022 L of O_{2} gas effuses in 1 hr

So, time taken for the effusion of 1.5 L of O_{2} gas is calculated as follows.

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3 years ago
If 100 ml of some pb(no3)2 solution is mixed with 100 ml of 6.50 x 10−2 m nacl solution, what is the maximum concentration of th
Alex73 [517]
Suppose X (in unit M) be the required maximum concentration of the Pb(NO₃)₂ solution added after mixing with 100 ml of 6.5 x 10⁻² M NaCl, the Pb²⁺ concentration is:
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The concentration of Cl⁻ is:
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So:
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X = (2.00 x 10⁻⁵) / (5.28 x 10⁻⁴) = 0.038 M
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