The solution contains 39.4% of LiF. Assume that the solution is 100ml. The molar mass of LiF is 25.939, the amount of LiF in mole would be: 100ml * 1g/ml * 39.4%/ 25.939g/mol= 1.52 mol LiF
Then the mass of the water would be: 100gram- 39.4g= 60.6g
If the molar mass of water is 18.015 the mole of the water would be: 60.6g/ 18.015g/mol= 3.36 mol
.
The mole fraction would be:1.52 mol/ 1.52+3.36= 0.339
Answer:
She will observe that the pressure on the tire is higher.
Explanation:
By the ideal gas law, the pressure and the temperature are directly proportional, so, if the temperature increases the pressure increases too:
PV = nRT (P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature).
The temperature is a measure of the average kinetic energy of the gas molecules, so when the temperature increases, the energy also increases, and the gas molecules will move more quickly, so they will collide more often between themselves and in the wall. Those collisions will be with more force because the velocity is higher.
So, the pressure will be higher, because it is the result of collisions of the gas molecules with the walls of the tire.
Answer:
Equilibrium constant is 0.0873
Explanation:
For the reaction:
A + B ⇄ C
Equilibrium constant is defined as:
K = [C] / [A] [B]
concentrations in equilibrium of each reactant are:
[A] = 10 - X
[B] = 5 - X
[C] = 15 + X
If concentration in equilibrium of B is 9, X is:
[B] = 5 - X = 9 → <em>X = -4 </em>
Replacing:
[A] = 10 - (-4) = 14
[B] = 5 - (-4) = 9
[C] = 15 + (-4) = 11
K = 11 / (14×9) = 0.0873
Thus, <em>equilibrium constant is 0.0873</em>
