Question

A sample of gas has a volume of 12.0 L at 0 c and 380 torr what will be it’s volume when the pressure is changed to 760 torr at constant temperature

Answer 1

Answer:The new volume would be 6 liters.

Step-by-step explanation:

PV=nRT

P is pressure in atm (760 torr = 1 atm);

V is volume in liters;

n is the number of moles;

R is the constant 0.0821;

T is temperature in Kelvin.

n, R, and T are constant; therefore,

P1V1=P2V2

Convert the torr into atm

P1 = 380torr/760torr×atm^−1

= 0.5 atm

P2 = 760torr/760torr×atm^−1

= 1 atm

Set the volume

V1 = 12 L

V2= x L

P1V1=P2V2

0.5atm×12L= 1atm×xL

xL = 6L

The new volume would be 6 liters.

Answer 2

To solve this problem, we can use the combined gas law, which relates the pressure, volume, and temperature of a gas:

P1V1/T1 = P2V2/T2

where P1, V1, and T1 are the initial pressure, volume, and temperature of the gas, respectively, and P2, V2, and T2 are the new pressure, volume, and temperature of the gas, respectively. Since the temperature is constant in this case, we can simplify the equation to:

P1V1 = P2V2

We can substitute the given values into the equation and solve for V2:

P1 = 380 torr

V1 = 12.0 L

P2 = 760 torr

Therefore:

V2 = (P1 x V1) / P2

V2 = (380 torr x 12.0 L) / 760 torr

V2 = 6.0 L

Therefore, the volume of the gas at a pressure of 760 torr is 6.0 L, assuming the temperature remains constant.

Step-by-step explanation: