The pressure in an automobile tire is 1.85 atm at 27.0°C. What will be the pressure if the temperature increases to 38.0°C?

I don't know if that 1.85 atm is absolute or not; I assume this is to be worked the "easier" way.

Use (p1/t1) = (p2/t2)
Don't forget T must be in kelvin.

To calculate the pressure in the tire at a different temperature, we can use the ideal gas law equation:

PV = nRT

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

First, we need to convert the given temperatures from Celsius to Kelvin. The Kelvin scale is an absolute temperature scale, so we add 273.15 to the Celsius temperature to get the corresponding temperature in Kelvin.

Given:
Temperature 1 (T1) = 27.0°C
Temperature 2 (T2) = 38.0°C

Converting to Kelvin:
T1 = 27.0 + 273.15 = 300.15 K
T2 = 38.0 + 273.15 = 311.15 K

Next, we need to assume that there is no change in the volume and amount of gas, so the equation becomes:

P1/T1 = P2/T2

Substituting the given values:
1.85 atm / 300.15 K = P2 / 311.15 K

Now, we can solve for P2, the pressure at the new temperature:

P2 = (1.85 atm * 311.15 K) / 300.15 K

Calculating this equation will give us the pressure in the tire at the new temperature.