Answer:
directly proportional to one another
Explanation:
Volatility refers to how quickly a substance changes from liquid to gas.
If a substance has a high vapour pressure, the substance is highly volatile. Similarly, if a substance has a low vapour pressure, then the substance is much less volatile.
This implies that volatility and vapour pressure gives a direct proportionality.
I’m pretty sure you would have to divide 5 and 30 and you will get 0.16666666 but I would think it would be 6cm/s but I could be wrong and if it is I’m am truly sorry.
To determine the amount of each solution that she should use, we do mass balance for the whole process. We let x be the amount the 65% salt and y the amount of the 90% salt. We do as follows:
The total mass should be equal to 150 oz.
x + y = 150
Doing a salt balance, we obtain the second equation:
.65x + .90y = 150(.85)
Solving for x and y, we obtain:
x = 30 oz
y = 120 oz
Answer:
Yes, there will be liquid present and the mass is 5.19 g
Explanation:
In order to do this, we need to use the equation of an ideal gas which is:
<em>PV = nRT (1)</em>
<em>Where:</em>
<em>P: Pressure</em>
<em>V: Volume</em>
<em>n: number of moles</em>
<em>R: gas constant</em>
<em>T: Temperature</em>
we know that the pressure is 856 Torr at 300 K. So, if we want to know if there'll be any liquid present, we need to calculate the moles and mass of the CCl3F at this pressure and temperature, and then, compare it to the initial mass of 11.5 g.
From (1), solving for moles we have:
<em>n = PV/RT (2)</em>
Solving for n:
P = 856/760 = 1.13 atm
R = 0.082 L atm / mol K
n = 1.13 * 1 / 0.082 * 300
n = 0.0459 moles
Now, the mass is:
m = n * MM (3)
The molar mass of CCl3F reported is 137.37 g/mol so:
m = 0.0459 * 137.37
m = 6.31 g
Finally, this means that if we put 11.5 g of CCl3F in a container, only 6.31 g will become gaseous, so, this means it will be liquid present, and the mass is:
m = 11.5 - 6.31
m = 5.19 g
The balanced chemical reaction would be
<span>pcl3(g) + cl2(g) = pcl5(g)
First, we need to determine the theoretical yield of the reaction assuming that all of the limiting reactant is used up. Then, we divide the actual yield to the theoretical yield to determine the percent yield.
Theoretical yield = 61.3 g Cl2 ( 1 mol / 70.9 g) ( 1 mol PCl5 / 1 mol Cl2 ) ( 208.2 g / 1 mol ) = 180.01 g PCl5
Percent yield = 119.3 g / 180.01 g x100 = 66.3%</span>
