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1.50 moles of N2 at 825 mmhg and 303 K are contained in a 34.3 L bottle. What is the pressure of the system if an additional 1.00 mole of gas is added to the bottle and the temperature is reduced to 273 K?

150 Moles Of N2 At 825 Mmhg And 303 K Are Contained In A 343 L Bottle What Is The Pressure Of The System If An Additional 100 Mole Of Gas Is Added To The Bottle class=

Sagot :

CrystalQueen

Answer:

1240 mmHg

Explanation:

Since volume is being held constant, we can use the following variation of the Ideal Gas Law to find the new pressure.

[tex]\frac{P_1}{T_1N_1}=\frac{P_2}{T_2N_2}[/tex]

In the equation, "P₁", "T₁", and "N₁" represent the initial pressure, temperature, and moles. "P₂", "T₂", and "N₂" represent the final pressure, temperature, and moles. Your answer should have 3 sig figs to match the sig figs of the given values.

P₁ = 825 mmHg                            P₂ = ? mmHg

T₁ = 303 K                                     T₂ = 273 K

N₁ = 1.50 moles                             N₂ = 1.50 + 1.00 = 2.50 moles

[tex]\frac{P_1}{T_1N_1}=\frac{P_2}{T_2N_2}[/tex]                                                     <----- Formula

[tex]\frac{825 mmHg}{(303K)(1.50 moles)}=\frac{P_2}{(273 K)(2.50 moles)}[/tex]                   <----- Insert values

[tex]\frac{825 mmHg}{454.5}=\frac{P_2}{682.5}[/tex]                                               <----- Simplify denominators

[tex]1.815=\frac{P_2}{682.5}[/tex]                                                     <----- Simplify left side

[tex]1238.86 mmHg={P_2}[/tex]                                          <----- Multiply both sides by 682.5

[tex]1240 mmHg={P_2}[/tex]                                              <----- Apply sig figs

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