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3 years ago

A 1.20-L container contains 1.10 g of an unknown gas at STP. What is the molecular weight of the unknown gas?

Chemistry

1 answer:

SOVA2 [1]3 years ago

8 0

Answer:

M = 20.5 g/mol

Explanation:

Given data:

Volume of gas = 1.20 L

Mass of gas = 1.10 g

Temperature and pressure = standard

Solution:

First of all we will calculate the density.

Formula:

d = mass/ volume

d = 1.10 g/ 1.20 L

d = 0.92 g/L

Now we will calculate the molar mass.

d = PM/RT

0.92 g/L = 1 atm × M / 0.0821 atm.L/mol.K ×273.15 K

M = 0.92 g/L × 0.0821 atm.L/mol.K ×273.15 K / 1 atm

M = 20.5 g/mol

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Explanation:

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3 years ago

The standard molar heat of fusion of ice is 6020 j/mol. calculate q, w, and ∆e for melting 1.00 mol of ice at 0◦c and 1.00 atm p

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Answer : q = 6020 J, w = -6020 J, Δe = 0

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Molar heat of fusion of ice = 6020 J/mole

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Pressure = 1 atm

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$q=\Delta H_{fusion}(\frac{Mass}{\text{ Molar mass}})$ (in terms of mass)

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Now we have to calculate the value of q.

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So, the value of $\Delta e=0$

Now we have to calculate the value of w.

Formula used : $\Delta e=q+w$

where, q is heat required, w is work done and $\Delta e$ is internal energy.

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3 years ago

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