A syringe of contains 589 mL of CO at 325 K and 1.2 atm pressure. A second syringe contains 473 mL of N2 at 298 K and 2.6 atm. What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at STP?
moles CO = pV/RT = 1.2 x 0.589 L/0.08206 x 325 = 0.0265
moles N2 = pV/RT = 2.6 x 0.473 L/ 0.08206 x 298= 0.0503
moles CO + moles N2 = 0.0265 + 0.0503 = 0.0768
at STP : T = 273 K
p = nRT/V = 0.0768 x 0.08206 x 273 / 1.00 L=1.7 atm
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