Respuesta :
Question is incomplete, complete question is :
A fixed quantity of gas at 21°C exhibits a pressure of 758 torr and occupies a volume of 5.42 L . Calculate the volume the gas will occupy if the pressure is increased to 1.89 atm while the temperature is held constant.
Answer:
The final volume of the gas will be 2.86 L.
Explanation:
initial pressure of the gas = [tex]P_1=758 Torr=\frac{758}{760} atm=0.997 atm[/tex]
initial volume of the gas = [tex]V_1=5.42 L[/tex]
Final pressure of the gas = [tex]P_2=1.89 atm[/tex]
Final volume of the gas = [tex]V_1=?[/tex]
Applying Boyle's law;
[tex]P_1V_1=P_2V_2[/tex] ( at constant temperature)
[tex]V_2=\frac{P_1V_1}{P_2}=\frac{0.997 atm\times 5.42 L}{1.89 atm}[/tex]
[tex]V_2=2.86 L[/tex]
The final volume of the gas will be 2.86 L.
The volume of gas occupied by increasing the pressure to 1.89 atm, while holding the temperature constant has been 2.86 L.
The question has given the temperature of 21 [tex]\rm ^\circ C[/tex], and the initial pressure of 758 torr. The initially has a volume of 5.42 L.
The final pressure has been given as 1.89 atm.
The initial pressure has been converted to atm units.
760 torr = 1 atm
758 torr = [tex]\rm \dfrac{758}{760}\;\times\;1[/tex] atm
758 torr = 0.997 atm
According to Boyle's law:
P1V1 =P2V2
Where, P1 and V1 are the initial pressure and volume respectively. P2 and V2 are the final pressure and volume respectively.
0.997 atm [tex]\times[/tex] 5.42 L = 1.89 atm [tex]\times[/tex] Final volume
Final volume = 2.86 L.
The volume of gas occupied by increasing the pressure to 1.89 atm, while holding the temperature constant has been 2.86 L.
For more information about the volume of gas, refer to the link:
https://brainly.com/question/2454734
