Answer:
a) increases
b) decreases
c) does not change
d) increases
Explanation:
The vapour pressure of a liquid is dependent on;
I) the magnitude of intermolecular forces
II) the temperature of the liquid
Hence, when any of these increases, the vapour pressure increases likewise.
Similarly, the boiling point of a liquid depends on the magnitude of intermolecular forces present because as intermolecular forces increases, more energy is required to break intermolecular bonds.
Lastly, increase in surface area of a liquid does not really affect it's vapour pressure.
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>
We are given with the percentage composition of oxygen in an oxide from phosphorus and oxygen equal to 43.6 percent. that is the phosphorus is equal to 56.4 percent. we divide each with the molar mass and divide each with the smaller quantity. P then is equal to 1 and O is equal to 1.5. In this case, the empirical formula is P2O3.
