Question

What volume would a gas occupy at 2 atm. And 227 °c if its volume at S. T. P is 2.5 litres

Answer 1

Explanation:

Hi there!

Here is the solution....⬇⬇

Let the initial volume be v1, pressure p1 and temperature t1, and the final volcano be v2, pressure p2 and temperature t2.

Therefore,

v1= 2.5 l

p1= 760 mmHg

t1= 273 K

and,

v2= v l

p2= 2 atm= 760 × 2 mmHg

t2= 227°C= (227+273)K = 500 K

Therefore, according to the Gas Equation,

\frac{p1 \times v1}{t1} = \frac{p2 \times v2}{t2}

= > \frac{760 \times 2.5}{273} = \frac{760 \times 2 \times v}{500}

= > v = \frac{760 \times 2.5 \times 500}{760 \times 2 \times 273}

= > v = 9.157509

I hope it helps you...

Answer 2

Answer:

P1=2atm V1=? T1=227+273=500k

P2=1atm T2=273K V2=2.5l

P1V1/T1=P2V2/T2

2×V1/500=2.5×1/273

V1=25×1×500/10×273×2

=625/273