Consider two empty containers a and b whose volumes are 10ml and 20ml respectively. 1ml of liquid water is put into each container and the temperature of each container is adjusted to 20°c. the gas pressure in container b, which still has some liquid water in it, is found to be 17 torr. how would the pressure in container a and the amount of liquid water in container a compare to that of container b?

The pressure in container A is higher than container B.

Explanation:

Applying ideal gas law PV=nRT, With the equation we can predict volume V is inverse to pressure P, that means if volume increase, pressure decrease.

The volume in container B is half A, that means respectively, pressure is the double.

check it with the equation:

n=1/18=0.05

R=62.36 L*Torr/K*mol

T=273+20=293 K

V=0.02 L

P=nRT/V =0.056*62.36*293/0.01=102.3 torr

I hope my answer helps you

the temperature of the gas, in k, not celsius.