Question #58008

A gas at 1.00 atm occupies 5.00 L. Under what pressure will the volume be 10.0 L if the temperature remains constant?

Expert's answer

The ideal gas law is written as:

PV = nRT

where n - number of moles of gas;

P - gas pressure (e.g., atm)

V - gas volume (liters);

T - gas temperature (in Kelvin);

R - gas constant (0.0821(L*atm)/(mol*K) )

n and T are constant, R is always constant

PV = constant

P1V1 = P2V2

1*5 = P2*10

P2 = 0.5 atm

Answer: Under the 0.5 atm pressure the volume will be 10.0 L

PV = nRT

where n - number of moles of gas;

P - gas pressure (e.g., atm)

V - gas volume (liters);

T - gas temperature (in Kelvin);

R - gas constant (0.0821(L*atm)/(mol*K) )

n and T are constant, R is always constant

PV = constant

P1V1 = P2V2

1*5 = P2*10

P2 = 0.5 atm

Answer: Under the 0.5 atm pressure the volume will be 10.0 L

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