An unscrupulous person, wanting to increase the horsepower of his muscle car, co

Question

An unscrupulous person, wanting to increase the horsepower of his muscle car, commandeers a full 5.00-L medical cylinder (P=204 atm at 25degree) and attaches it with a metering valve to the air intake of his engine, The N2O liberates energy by decomposition according to: N20 rightarrow N2 + 1/2 02 + 82 kj How much heat would be released into the combustion chambers of his engine if all of the N2 in the cylinder were to be injected into the engine, if no work were done by or on the system (i.e. at constant P and T? A hyperbaric chamber with an empty volume of 1,530 L was filled with 9,180 L of a gas mixture originally at a temperature of 298.15 K and pressure of 0.9907 atm. The gas mixture contained 75.0% O2 and 25.0% N2 by volume, and was used to treat a patient with carbon monoxide poisoning

Explanation / Answer

First calculate the number of moles from the use of gas law:

PV= nRT

n= PV/RT

n= 204 atm * 5.00 T / 0.082057 L atm mol-1K-1*298 K

n= 41.7 mol

one mol N2O gives = 82 KJ

41.7 mol N2O will give= 82 KJ *41.7 mol =3420.3 KJ

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