What is the nature of the Ca-Cl bond in a molecule of calcium chloride (CaCl2) if the electronegativity value of calcium is 1.0
and that of chlorine is 3.16?
1 answer:
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Answer:
The heat at constant pressure is -3,275.7413 kJ
Explanation:
The combustion equation is 2C₆H₆ (l) + 15O₂ (g) → 12CO₂ (g) + 6H₂O (l)
= (12 - 15)/2 = -3/2
We have;
Where R and T are constant, and ΔU is given we can write the relationship as follows;
Where;
H = The heat at constant pressure
U = The heat at constant volume = -3,272 kJ
= The change in the number of gas molecules per mole
R = The universal gas constant = 8.314 J/(mol·K)
T = The temperature = 300 K
Therefore, we get;
H = -3,272 kJ + (-3/2) mol ×8.314 J/(mol·K) ×300 K) × 1 kJ/(1000 J) = -3,275.7413 kJ
The heat at constant pressure, H = -3,275.7413 kJ.
Answer:
Explanation:
Hello there!
In this case, when considering weak acids which have an associated percent dissociation, we first need to set up the ionization reaction and the equilibrium expression:
Now, by introducing x as the reaction extent which also represents the concentration of both H+ and A-, we have:
Thus, it is possible to find x given the pH as shown below:
So that we can calculate the initial concentration of the acid:
Therefore, the percent dissociation turns out to be:
Best regards!