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ki77a [65]
3 years ago
8

a 108ml sampl of gas has a mass of 77.96mg at a pressure of 1140mmhg and temperature of 183°c .what is the molar mass of the gas

?​
Chemistry
2 answers:
liq [111]3 years ago
5 0

Answer:

Molar mass = 20 g/mol

Explanation:

Given data:

Volume of gas = 108 mL

Mass of gas = 77.96 mg (77.96/1000 = 0.08 g)

Pressure of gas = 1140 mmHg

Temperature of gas = 183°C

Molar mass of gas = ?

Solution:

First of all we will calculate the number of moles of gas.

PV = nRT

R = general gas constant = 0.0821 atm.L/ mol.K

Now we will convert the units and then we will put the values in formula.

Volume of gas = 108 mL× 1 L/1000 mL= 0.108 L

Pressure of gas = 1140 mmHg× 1 atm / 760 mmHg = 1.5 atm

Temperature of gas = 183+273 = 456 K

PV = nRT

1.5 atm ×0.108 L = n × 0.0821 atm.L/ mol.K ×456 K

0.162 atm.L =  n ×37.44 atm.L/ mol

n = 0.162 atm.L/37.44 atm.L/ mol

n = 0.004 mol

Molar mass of gas:

Number of moles = mass/molar mass

0.004 mol = 0.08 g / molar mass

Molar mass = 0.08 g /0.004 mol

Molar mass = 20 g/mol

madam [21]3 years ago
3 0

Answer:

146.85 g/mol

Explanation:

PV=nRT

n=mass/molar mass

covert from mmhg to atm = 0.184 atm

convert from ml to L= 0.108 L

convert from degree C to K= 456.15 K

convert from mg to g= 0.07796g

then rearrange the formula:

n=PV/RT

=(0.184)(0.108)/(0.08206)(456.15)

n= 5.308*10^(-4)

rearrange the n formula interms of molar mass:

Molar mass= mass/n

=0.07796/(5.308*10^-4)

molar mass= 146.85g/mol

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Molar mass of [Co(NH_3)_4(H_2O)_2]Cl_2 = 234 g/mol

Moles of [Co(NH_3)_4(H_2O)_2]Cl_2 = 0.0168 moles

Putting values in equation 1, we get:

0.0168mol=\frac{\text{Mass of }[Co(NH_3)_4(H_2O)_2]Cl_2}{234g/mol}\\\\\text{Mass of }[Co(NH_3)_4(H_2O)_2]Cl_2=(0.0168mol\times 234g/mol)=3.93g

To calculate the percentage yield of [Co(NH_3)_4(H_2O)_2]Cl_2, we use the equation:

\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100

Experimental yield of [Co(NH_3)_4(H_2O)_2]Cl_2 = 1.20 g

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