Respuesta :

Skinider
Given; 
no. of moles (n) = 500 moles
volume (V) = 1.2 l
temperature (T) = 150°C = (150 + 273 )k = 423 k
gas constant (R) = 0.0821 L- atm / mole-K

then,

PV = nRT
P × 1.2 = 500 × 0.0821 × 423
P =  14,470.125 atm

But I guess pressure is too high. Well this should be the way.
Eduard22sly

The pressure of the ammonia inside the flask is 14470.125 atm

From the question given above, the following data were obtained:

  • Number of mole (n) = 500 moles
  • Volume (V) = 1.2 L
  • Temperature (T) = 150 °C = 150 + 273 = 423 K
  • Gas constant (R) = 0.0821 atm.L/Kmol
  • Pressure (P) =?

Using the ideal gas equation, the pressure of the ammonia inside the flask can be obtained as follow:

PV = nRT

P × 1.2 = 500 × 0.0821 × 423

P × 1.2 = 17364.15

Divide both side by 1.2

P = 17364.15 / 1.2

P = 14470.125 atm

Thus, the pressure of the gas in the flask is 14470.125 atm.

Learn more about ideal gas equation:

https://brainly.com/question/4147359

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