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Answer:
The total pressure is 1.616 atm
Explanation:
First of all we say:
In a closed system, sum of partial pressures is the value for the total pressure.
In our system, we have gas A and B
Total pressure without the third gas is = 0.373 atm + 0.650 atm = 1.023 atm
As we add a third gas, with no change in volume or T°, let's find out by the Ideal Gases Law, its pressure:
P . V = n . R . T
P = ( n . R . T) / V
P = (0.220 mol . 0.082 . (273 + 21°C)) / 8.95L = 0.593 atm
273 + 21°C → Absolute value of T°
Let's sum the partial pressures, then:
0.373 atm + 0.650 atm + 0.593 atm = 1.616 atm.
It's ok to say that the total pressure was increased, because we have more gas now.
This can be done in the following way;
1 determining the heat required to convert 0° C ice to 0°C water
Heat of fusion of water = 334 J/g
Therefore; Heat = 50 g × 334 J/g = 16700 J
2. Determining the heat required to raise the temperature of water from 0° C to 100°C.
Specific heat of water is 4.18 J/g°C
Change in temperature is 100°C
Therefore; Heat = 50 g × 4.18 J/g°C × 100 = 20900 J
3. Determining the heat required to convert 100 ° C water to 100°C vapor
Heat of vaporization of water = 2257 J/g
Heat = Mass of water × heat of vaporization
Heat = 50 g × 2257 = 112850 J
4. Determining the heat required to go from 100° C to 120° vapor
specific heat of vapor = 2.09 J/g°C
Heat = mass × Specific heat of vapor × change in temperature
= 50 g × 2.09 ×(120-100) = 2090 J
Therefore the total heat required is
= 16700 J + 20900 J + 112850 J + 2090 J = 152540 J or 152.54 kJ
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