Question

Someone hands you a sample of carbon monoxide with a pressure of 11.83kpa a volume of 1.27L and a temperature of 330.6K. If you double the pressure and reduce the temperature to 149.9K what will the resulting volume of the gas be in liters?

Answer 1

The final volume of the gas is 0.29 L

Step-by-step explanation:

Here, we want to get the final volume of a given mass of gas

From the question, we are given the initial condition values, and we want to get the final volume

The gas law to use is the general gas law

We have the mathematical representation as follows:

`\frac{P_iV_i}{T_i\text{ }}\text{ = }(P_fV_f)/(T_f)`

While i represents the intial values, the f values represents the final values

Let us get the values as given in the question

Initial values:

Pressure = 11.83 kPa

Volume = 1.27 L

Temperature = 330.6 K

Final values;

Pressure = 2(11.83) kPa : The pressure value was doubled

Volume = ?

Temperature = 149.9 K

We proceed to substitute these values into the equation written above

We have this as follows:

`(11.83*1.27)/(330.6)\text{ = }(2(11.83)* V)/(149.9)`

Finally, we get the volume value as follows:

`V\text{ = }(11.83*1.27*149.9)/(330.6*2(11.83))\text{ = 0.29 L }`