a car tyre pumped in the morning at 10°C to a pressure of 0.2N per mm²,increases in pressure as temperature rises. If the temperature is18°C,whatis the new pressure,the volume is constant.
P1V1/T1=P2V2/T2
Solve for P2
Volumes are constant and cancel out.
Use C° + 273K=???? To convert C° to Kelvin....
Are the three "anonymous" the same person. At any rate the last two posts are the corect way to go. Follow up if the first anonymous still has questions.
To find the new pressure of the car tire, we can use the ideal gas law, which states that the pressure of a gas is directly proportional to its temperature.
Step 1: Convert temperatures to Kelvin
To use the ideal gas law equation, we need to convert the temperatures from Celsius to Kelvin. The relationship between Celsius (°C) and Kelvin (K) is K = °C + 273.15.
Initial temperature (T1) in Kelvin:
T1 = 10°C + 273.15 = 283.15 K
Final temperature (T2) in Kelvin:
T2 = 18°C + 273.15 = 291.15 K
Step 2: Set up the equation
The ideal gas law equation is: P1/T1 = P2/T2
where P1 and T1 are the initial pressure and temperature, respectively, and P2 and T2 are the final pressure and temperature, respectively.
Step 3: Solve for P2
P1/T1 = P2/T2
Substituting the given values:
0.2 N/mm² / 283.15 K = P2 / 291.15 K
Step 4: Calculate the new pressure (P2)
Cross-multiply and solve for P2:
P2 = (0.2 N/mm²)(291.15 K) / 283.15 K
P2 ≈ 0.206 N/mm²
Therefore, the new pressure of the car tire at 18°C is approximately 0.206 N/mm².