Question

A sample of gas at 1.2 atm and 27°C is heated at constant pressure to 57°C. Its final volume is found to be 4.75 litres. What was its original volume?

Answer 1

apply the charles law
v/t of the first gas =v/t of the second
v/300=4.75/330
4.31 l

Answer 2

Given:

Final volume = 4.75 L

Initial temperature = 27°C = 300K

Final temperature = 57°C = 330K

To find:

Initial volume ($V_1$) = ?

Formula to be used:

$\frac{V_1}{T_1} = \frac{V_2}{T_2}$

Calculation:

$\frac{V_1}{T_1} = \frac{V_2}{T_2}$

Substituting the given values in the following formula gives

$\frac{V_1}{300K} = \frac{4.75}{330K}$

$V_1$ = $\frac{4.75\times 300}{330}$

$V_1 = \frac{4.75\times 10}{11}$

$V_1 = \frac{47.5}{11}$

$V_1$ = 4.318

Conclusion:

The original volume of the gas was calculated as 4.3 L.

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