Answer:
new solubility = 0.443 g/l
Explanation:
To solve this question, we will use Henry's law.
Henry's law states that, at constant temperature:
S1 / P1 = S2 / P2
We are given that:
S1 = 0.16 g/l
P1 = 104 kPa
S2 is the solubility we want to calculate
P2 = 288 kPa
Substitute with the givens in the above relation to get the new solubility (S2) as follows:
0.16 / 104 = S2 / 288
S2 = (0.16/104) * 288
S2 = 0.443 g/l
Hope this helps :)
Answer:
I. Increasing pressure will allow more frequent successful collision between particles due to the particles being closer together.
II. Rate of reaction increases due to more products being made; as increased pressure favours the exothermic side of the equilibrium.
III. Increasing temperature provides particles lots of (Kinetic) energy, for more frequent successful collision due to the particles moving at a faster rate than before. However, favouring the endothermic side of the equilibrium due to lots of energy required to break and form new bonds.
IV. Rate of reaction increases due to increase temperature favouring both directions of the equilibrium - causing products to form faster.
Hope this helps!
Answer:
true
Explanation:
because if you find the right answer that proves the theory to be correct.
To answer this item, we determine first the number of moles of O2 produced.
n = (250 g O2) / (32 g O2/mol) = 7.8125 moles O2
From the given balanced chemical equation, every one mole of O2 needs 2 moles mercury oxide.
n HgO = (7.8125 moles O2) x (2 moles HgO / 1 mole O2)
n HgO = 15.625 moles O2