Question

The volume and the amount of gas are constant in a tire. The initial pressure and temperature are 1.82 atm and 293 K. At what temperature will the gas in the tire have a pressure of 2.35 atm?

What gas law will you use to solve this problem?The value for P1 is
, the value for P2 is
, the value of T1 is
, and the value for T2 is
. What Kelvin temperature will the gas in the tire have when the pressure is increased?
.

HELP PLS

Answer 1

To solve this problem, we can use the ideal gas law:

PV = nRT

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

Since the volume and the amount of gas are constant in this problem, we can use the following equation to find the relation between the pressure and temperature:

P1/T1 = P2/T2

where P1 and T1 are the initial pressure and temperature, and P2 is the pressure at the unknown temperature T2.

Substituting the given values, we have:

1.82 atm / 293 K = 2.35 atm / T2

Solving for T2, we get:

T2 = 1.82 atm * 293 K / 2.35 atm = 227.37 K

Therefore, the gas in the tire will have a temperature of 227.37 K, or approximately -45.78 degrees Celsius, when the pressure is increased to 2.35 atm.