Answer:
To solve this problem, we can use the ideal gas law, which relates the pressure, volume, number of moles, and temperature of a gas:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
We are given:
P1 = 1.88 atm
T1 = 25.0°C = 298.15 K
We need to find P2, given:
T2 = 37.0°C = 310.15 K
We can assume that the volume and number of moles of gas remain constant.
Substituting these values into the ideal gas law equation, we get:
P1V = nRT1
P2V = nRT2
Dividing the second equation by the first equation, we get:
P2/P1 = T2/T1
Substituting the values we have, we get:
P2/1.88 atm = 310.15 K/298.15 K
Solving for P2, we get:
P2 = (1.88 atm) x (310.15 K)/(298.15 K) = 1.96 atm
Therefore, the pressure in the tire will be 1.96 atm if the temperature warms up to 37.0°C.