A car tyre pump in the morning at 10degree celcius to a pressure of 0.20NM/S increases in pressure at it's temperature rises.if the temp. reachs 18degree celcius,what is the pressure
Again use
P1V1/T1=P2V2/T2, where V is constant
P1/T1=P2/T2
The units of P do not matter (I don't understand yours) as you can quote the found pressure in the units given in the question. Remember to convert deg C to K.
Thank U
To find the final pressure, we need to use the ideal gas law formula, which states:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature in Kelvin
First, let's convert the temperatures from Celsius to Kelvin:
Initial temperature: 10°C + 273.15 = 283.15 K
Final temperature: 18°C + 273.15 = 291.15 K
Since the volume and the number of moles remain constant, we can simplify the formula to:
P1/T1 = P2/T2
Where:
P1 = initial pressure
T1 = initial temperature in Kelvin
P2 = final pressure
T2 = final temperature in Kelvin
Now we can plug in the values and solve for P2:
P1/T1 = P2/T2
P1 = 0.20 N/m^2 (given)
T1 = 283.15 K (initial temperature)
T2 = 291.15 K (final temperature)
0.20 N/m^2 / 283.15 K = P2 / 291.15 K
Now we can solve for P2:
P2 = (0.20 N/m^2 / 283.15 K) * 291.15 K
P2 ≈ 0.2049 N/m^2
Therefore, when the temperature reaches 18°C, the pressure will be approximately 0.2049 N/m^2.
To determine the pressure of the car tire pump when the temperature reaches 18 degrees Celsius, we need to consider the relationship between temperature and pressure in gases.
The relationship between temperature and pressure is described by the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
In this case, we are given the initial pressure and temperature, but we do not have the volume or the number of moles. However, since we only need to compare the pressure at two different temperatures, we can assume that the volume and the number of moles remain constant.
So, let's convert the temperatures from Celsius to Kelvin:
Initial temperature = 10 degrees Celsius + 273.15 = 283.15 K
Final temperature = 18 degrees Celsius + 273.15 = 291.15 K
Now we can set up a ratio using the ideal gas law:
(P1 * V) / T1 = (P2 * V) / T2
Since we assume that the volume and the number of moles remain constant, we can cancel them out of the equation.
(P1 / T1) = (P2 / T2)
We have the initial pressure (P1) as 0.20 N/m^2 (assuming NM/S is a typo) and the initial temperature (T1) as 283.15 K. We need to solve for the final pressure (P2) when the temperature (T2) is 291.15 K.
(P1 / T1) = (P2 / T2)
(0.20 N/m^2 / 283.15 K) = (P2 / 291.15 K)
We can cross-multiply and solve for P2:
(0.20 N/m^2 * 291.15 K) / 283.15 K = P2
P2 ≈ 0.206 N/m^2
Therefore, when the temperature reaches 18 degrees Celsius, the pressure of the car tire pump will be approximately 0.206 N/m^2.