Question

to what temperature must a sample of nitrogen at 27 degrees C and 0.625atm be taken so that its preassure becomes 1.125atm at constant volume?​

Answer 1

540k or 267°C

Explanation:

Given parameters:

T1 = 27°C

P1 = 0.625atm

P2 = 1.125atm

condition = constant volume

Unknown:

T2 = final temperature = ?

Solution:

From the combined gas law, if we assume that the condition is under a constant volume, the pressure of a given mass of gas will vary directly as the absolute temperature;

      $\frac{P1}{T1} = \frac{P2}{T2}$

P1 is the initial pressure

T1 is the initial temperature

P2 is the final pressure

T2 is the final temperature

 Now convert the given temperature to kelvin;

  tK = 273 + 27 = 300K

  Input the values in the equation;

    $\frac{0.625}{300} = \frac{1.125}{T2}$

  T2 = 540k or 267°C

learn more:

Ideal gas law brainly.com/question/13064292

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