Answer:
Vapor pressure of solution is 78.2 Torr
Explanation:
This is solved by vapor pressure lowering:
ΔP = P° . Xm . i
Vapor pressure of pure solvent (P°) - vapor pressure of solution = P° . Xm . i
NaCl → Na⁺ + Cl⁻ i = 2
Let's determine the Xm (mole fraction) These are the moles of solute / total moles.
Total moles = moles of solvent + moles of solute
Total moles = 0.897 mol + 0.182 mol → 1.079 mol
0.182 / 1.079 = 0.168
Now we replace on the main formula:
118.1° Torr - P' = 118.1° Torr . 0.168 . 2
P' = - (118.1° Torr . 0.168 . 2 - 118.1 Torr)
P' = 78.2 Torr
Answer:
The answer to your question is 6.77 atm
Explanation:
Data
Pressure 1 = P1 = 7.5 atm
Temperature 1 = T1 = 65°C
Pressure 2 = P2 = ?
Temperature 2 = T2 = 32°C
Process
-Use Gay-Lussac law to solve this problem
P1/T1 = P2/T2
-Solve for P2
P2 = P1T2 / T1
-Convert temperature to °K
T1 = 65 + 273 = 338°K
T2 = 32 + 273 = 305°K
-Substitution
P2 = (7.5 x 305) / 338
-Simplification
P2 = 2287.5 / 338
-Result
P2 = 6.77 atm
Angle of Solar Radiation and Temperature
Haber process is the large scale manufacture of a ammonia by reacting nitrogen and hydrogen at a ratio of 1:3
Change in hydrogen concentration is 0.45 - 0.16 = 0.29 moles/l
Therefore, the average rate of reaction of hydrogen = 0.29 / 30 = 0.0096
= 0.0096 moles/liter/sec
1. First, you have to find the number of moles 1.6z10^5L of gas is at 373K and 0.967atm using PV=nRT solving for n. (n=PV/RT). Everything is in the correct units and we know R is going to be 0.08206atmL/molK since it is a constant.
n=(0.967atmx160000L)/(0.08206atmL/molKx373K)
n=5054.8mol gas
Then you have to find the the number grams which can be found using the molar mass given as 29g/mol. multiply 29g/mol by the number of moles of gas we found in the previous step.
5054.8molx29g/mol=146589.9g of gas
Lastly, to find the density of the gas you need to divide the mass of the gas by its volume.
146589.9g/160000L=0.916g/L
2. The dinsity of the gas at STP should be higher than the density of gas with the given conditions. This is due to the fact that the given conditions involves a higher temperature than that of at STP which will cause the gas to expand therefore increasing the volume with out increasing the mass. The reason why the pressure is not building up even though the pressure is higher is that the balloon is not sealed meaning the gas can maintain about atmospheric pressure while expanding since the excess are just leaves the balloon.
the answer to part 2 can be proven by the fallowing:
To find the density of the gas at STP you first multiply the molar volume of gas at STP by the number of moles of gas from part 1 to get the volume of the gas at STP.
5054.8molx22.4L/mol=113228L
Then you divide the mass form part by the new volume to get the new density.
<span>146589.9g/113228L=1.30g/L</span>
I hope this helps. Let me know in the comments if any of it is unclear.
