t 103


C, the pressure of a sample of nitrogen
is 1
.
89 atm. What will the pressure be at
275

C, assuming constant volume?
Answer in units of atm

To answer this question, we can make use of the Ideal Gas Law, which states that the pressure of a gas is directly proportional to its temperature (in Kelvin) when the volume and the amount of gas are kept constant. The equation for the Ideal Gas Law is:

PV = nRT

Where:
P = pressure
V = volume
n = amount of gas (in moles)
R = ideal gas constant
T = temperature (in Kelvin)

First, let's convert the initial temperature from Celsius to Kelvin. We can do this by adding 273.15 to the Celsius temperature:

T1 = 103 + 273.15 = 376.15 K

Next, let's find the pressure at a new temperature of 275 °C, which can also be converted to Kelvin:

T2 = 275 + 273.15 = 548.15 K

Since the volume is assumed to be constant, we can rearrange the Ideal Gas Law equation to solve for the final pressure:

P1/T1 = P2/T2

Now, substitute the known values:

1.89 atm / 376.15 K = P2 / 548.15 K

To solve for P2 (the pressure at 275 °C), cross-multiply and then divide:

P2 = (1.89 atm) * (548.15 K) / 376.15 K

Calculating this expression gives us:

P2 ≈ 2.76 atm

Therefore, assuming constant volume, the pressure of the nitrogen gas at 275 °C would be approximately 2.76 atm.