Question

0.25 moles of a gas at 760 mmHg

and 298 K are contained in a 6.1 L
bottle. What is the pressure of the
system if the amount of gas in the
bottle is reduced to 0.13 mole and
the temperature is reduced to 100 K?

Answer 1

132.62

Step-by-step explanation:

i got the answer correct in the program

Answer 2

Answer: 2.3*10^3 Pa.

Explanation: We can use the ideal gas law to determine the pressure of the system: PV = nRT

where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

The ideal gas constant R = 8.314 J/mol*K

Given:

n1 = 0.25 moles

V1 = 6.1 L

T1 = 298 K

P1 = 760 mmHg

n2 = 0.13 moles

V2 = 6.1 L

T2 = 100 K

We can use the equation PV = nRT to find the new pressure P2, using the information provided:

P2 = (n2RT2)/V2

We know that the volume of the bottle remains the same and we can convert the pressure from mmHg to Pascals

P2 = (0.138.314100)/6.1 = 2.3*10^3 Pa

Therefore, the pressure of the system when the amount of gas in the bottle is reduced to 0.13 mole and the temperature is reduced to 100 K is 2.3*10^3 Pa.