Question

A gas has a volume of 300 ml at 27°C and 730mm(hg) pressure . What will be its volume at standard condition of temperature and pressure​

Answer 1

Primary Temperature ( T₁ ) = 27°C = ( 273 + 27 ) K = 300 K

Primary Pressure ( P₁ ) = 730 mm Hg

Primary Volume ( V₁ ) = 300 ml

And ,

Secondary Pressure ( P₂ ) = 760 mm Hg

Secondary Temperature ( T₂ ) = 273 K

Let , the volume be ( V₂ ) = V₂

•°• Therefore we know ,

P₁V₁ / T₁ = P₂V₂ / T₂

V₂ = P₁V₁T₂ / T₁P₂

V₂ = ( 730 × 300 × 273 ) / ( 300 × 760 )

V₂ = 73 × 273 / 76

V₂ = 73 × 3.59

V₂ = 262.07. [ • Required Answer]

•°• The volume of the gas will be 262.07 ml

Answer 2

The volume at standard condition of temperature and pressure​ is 262 ml.

Explanation:

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

where,

$P_1$ = initial pressure of gas = 730 mm of Hg

$P_2$ = final pressure of gas (at STP) = 760 mm of Hg

$V_1$ = initial volume of gas = 300 ml

$V_2$= final volume of gas (at STP) = ?

$T_1$ = initial temperature of gas = $27^0C=(27+273)K=300K$

$T_2$ = final temperature of gas (at STP) = 273 K

Now put all the given values in the above equation, we get:

$\frac{730\times 300}{300K}=\frac{760\times V_2}{273K}$

$V_2=262ml$

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