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antoniya [11.8K]
3 years ago
8

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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a) ΔHºrxn = 116.3 kJ, ΔGºrxn = 82.8 kJ,  ΔSºrxn =  0.113 kJ/K

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a)                                 C6H5−CH2CH3  ⇒  C6H5−CH=CH2  + H₂

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ΔHºrxn = 116.3 kJ

Similarly,

ΔGrxn = ΔGºf C6H5−CH=CH2 +  ΔGºfH₂ - ΔGºfC6H5CH2CH3

ΔGºrxn=   202.5 kJ + 0 kJ - 119.7 kJ  = 82.8 kJ

ΔSºrxn = 238 J/mol + 130.6 J/mol -255 J/K = 113.6 J/K = 0.113 kJ/K

b) The temperature at which the reaction is spontaneous or feasible occurs when ΔG becomes negative and using

ΔGrxn =  ΔHrxn -TΔS

we see that will happen when the term  TΔS  becomes greater than ΔHrxn since ΔS  is positive  , and so to sollve for T we will make ΔGrxn equal to zero and solve for T. Notice here we will make the assumption that  ΔºHrxn and ΔSºrxn remain constant at the higher temperature  and will equal the values previously calculated for them. Although this assumption is not entirely correct, it can be used.

0 = 116 kJ -T (0.113 kJ/K)

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to calculate ΔGrxn   with the assumption that ΔHº and ΔSºremain constant.

ΔG =  116.3 kJ - (600+273 K) x 0.113 kJ/K =  116.3 kJ - 873 K x 0.113 kJ/K

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ΔG = -RTlnK and solve for K

- ΔG / RT = lnK  ∴ K = exp (- ΔG / RT)

K = exp ( - 1.8 x 10⁴ J /( 8.314 J/K  x 873 K)) = 8.2 x 10⁻²

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