Answer:
There are exactly 5
Explanation:
IF YOU BREAK IT UP IT WILL BE FIVE
Answer:
pH = 1.32
Explanation:
H₂M + KOH ------------------------ HM⁻ + H₂O + K⁺
This problem involves a weak diprotic acid which we can solve by realizing they amount to buffer solutions. In the first deprotonation if all the acid is not consumed we will have an equilibrium of a wak acid and its weak conjugate base. Lets see:
So first calculate the moles reacted and produced:
n H₂M = 0.864 g/mol x 1 mol/ 116.072 g = 0.074 mol H₂M
54 mL x 1L / 1000 mL x 0. 0.276 moles/L = 0.015 mol KOH
it is clear that the maleic acid will not be completely consumed, hence treat it as an equilibrium problem of a buffer solution.
moles H₂M left = 0.074 - 0.015 = 0.059
moles HM⁻ produced = 0.015
Using the Henderson - Hasselbach equation to solve for pH:
ph = pKₐ + log ( HM⁻/ HA) = 1.92 + log ( 0.015 / 0.059) = 1.325
Notes: In the HH equation we used the moles of the species since the volume is the same and they will cancel out in the quotient.
For polyprotic acids the second or third deprotonation contribution to the pH when there is still unreacted acid ( Maleic in this case) unreacted.
Sulfur + oxygen --> sulfur dioxide
Answer:
ΔS = 16.569 J/K
Explanation:
In this case, we need to use the correct expression to solve this. In thermodynamics, the expression to use that puts a relation between heat, temperature and entropy is the following:
ΔS = Q/T
To determine the entropy change of the universe, we need to sum the entropy change of Earth and the entropy of the sun.
As the sun is transfering radiation to Earth, the sun is losing energy, therefore, heat is negative, while Earth receives the heat, so it's positive. Calculating the entropy for the sun and Earth:
ΔSs = -Q/Ts
ΔSe = Q/Te
ΔSu = ΔSe + ΔSs
Let's calculate both entropies by separate:
ΔSe = 5x10^3 / 285 = 17.54 J/K
ΔSs = -5x10^3 / 5,150 = -0.971 J/K
Therefore, the entropy of universe:
ΔSu = 17.54 - 0.971
ΔSu = 16.569 J/K
