Question

A gas is found with an unknown volume at a pressure of 1.5 atm and a temperature of 325K If the pressure is raised to 1.2 atm, the temperature is decreased to , 320K and the final volume is measured to 48 liters, what was the initial volume of the gas? 110 L 121 39 T. 42 L

Answer 1

The initial volume of the gas is 39 L, option C is the correct answer

What is the combined Gas Law?

According to combined gas law,

PV= nRT

In the Combined Gas Law, if we change either one of the variables the others will also change.

Here , Pressure (P), volume (V), number of mole of gas (n), and temperature (T).

When the moles of the gas is constant , the above equation can be written as ,

$\rm\dfrac{P'V'}{T'} = \dfrac{PV}{T}$

The data given in the question is

P = 1.5 atm

V=  ? ml

T=325 K

V'= 48 L

P'= 1.2 atm

T' =320 K

Substituting the values in the above formula

$\rm\dfrac{1.2\times\;48}{320} = \dfrac{1.5\;\times V}{325}$

$\rm\dfrac{1.2\times\;48}{320} = \dfrac{1.5\;\times V}{325}\\\\\\\;\;\;\;\;\;V= 39 \;L$

Therefore the initial volume of the gas is 39 L, option C is the correct answer

To know more about Combined Gas Law:

brainly.com/question/13154969

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