For a 0.00554 mol sample of H2, P=23.44 torr and T=557 K. What is its volume?

The volume is 8,22 liters.

Explanation:

The unit of pressure (from Torr to atm) must be converted: 760 Torr = 1 atm

760 Torr---1 atm

23,44Torr--x= (23,44Torr x 1 atm)/760 Torr= 0,0308 atm

PV=nRT V= (nRT)/P

V=(0,00554 mol x 0,082 l atm/K mol x 557 K)/ 0,0308 atm

V=8, 22 L

while cooking a piece of 1/2 pound beef steak, a cast iron pan (2.4kg in weight) was heated 260 celsius.

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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