A syringe contains 589 mL of CO at 325 K and 1.2 atmpressure. A second syringe c

Question

A syringe contains 589 mL of CO at 325 K and 1.2 atmpressure. A second syringe contains 473 mL of N2 at 298K and 2.6 atm.
a) How many moles of gas are in each syringe? i got .0265 for O2 and .0503 Mole of NH3.
b)What is the final pressure if the contents of thesetwo syringes are injected into a 1.00 L container at 298K? i got .0768 atm.
c) when an appropriate catalst is introduced to the gas mixture in part (a), NH3 and O2 react to form gaseous N2O and gaseous H2O. With the starting conditions from part (b), what is the partial pressure of each gas remaining in the mixture after the reaction goes to completion at 298K?
What is the total pressure?
d) comment on the total pressure in the 1.00 L bottle before and after the reaction. How did the pressure change of the course of the reaction? Why did it change in that way?

Explanation / Answer

pV/RT

= 1.2 x 0.589 L/0.08206 x 325

= 0.026 (moles CO )

pV/RT

= 2.6 x 0.473 L/ 0.08206 x 298

= 0.0503 (moles N2)

0.0265 + 0.0503

= 0.076

p = nRT/V

= 0.0768 x 0.08206 x 273 / 1.00 L

=1.7 atm

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