Need some Chemistry Help, Please

Question

1)When the vapor pressure of water is 149.4 torr, the temperature of the waters is?

2)A mixture of oxygen and nitrogen gas is reacted with white phosphorus to remove the oxygen. The volume decreases from 50.0 mL to 35.0 mL and the pressure remains constant at 740 torr. What was the original partial pressure (in torr) of oxygen assuming that the temperature has remained constant?

(Atomic weights: O = 16.00, N = 14.01).

I need explanations please, i'd really appreciate it

Answer 1

When the vapor pressure of water is 149.4 torr, the temperature of the waters is?

Your answer is: 60 drgrees Celsius

& that's from the CRC handbook of chemistry & physics,

or did you want it calculated using the Clausius-Clapeyron equation

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2)A mixture of oxygen and nitrogen gas is reacted with white phosphorus to remove the oxygen. The volume decreases from 50.0 mL to 35.0 mL and the pressure remains constant at 740 torr. What was the original partial pressure (in torr) of oxygen assuming that the temperature has remained constant?

but if the volume had not decreased, but had remained at 50ml ,... the pressure would have dropped by an amount equal to the partial

pressure of oxygen.

But we are talking a 30% drop in volume to go from 50 to 35 ml,,,,(15ml / 50ml)..... & that happened because oxygen was 30% of the total pressure , & now its gone:

30% of 740 Torr is 222 torr

your answer is : O2 was 222Torr of the original 740