Question

A tire has a pressure of 325 kPa at 10°C. If the temperature of the tire rises to 50°C and the volume remains constant, what is the new pressure? (Hint: °C + 273 = K.)

Answer 1

Multiply 325by 10c then multiply 50c the c will be 10c and the k will be283

Answer 2

The new pressure is 285 kPa

Step-by-step explanation:

Given:

Initial pressure of the tire, P1 = 325 kPa

Initial Temperature, T1 = 10 C

Final Temperature, T2 = 50 C

To determine:

The final pressure of the tire, P2

Step-by-step explanation:

Based on the ideal gas equation

`PV = nRT`

where P = pressure, V = volume ; n = moles of gas

R = gas constant, T = temperature

At constant n and V, the above equation becomes:

P/T = constant

This is the Charles law

Therefore:

`(P1)/(T1) = (P2)/(T2) \\\\P2 = (P1)/(T1) *T2 = (325 kPa*(10+273)K)/((50+273)K) =285 kPa`