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ser-zykov [4K]
3 years ago
6

Consider this equilibrium for a buffer solution: CH3COOH + H2O CH3COO- + H3O + . When a small amount of acid is added to this sy

stem, which statement is true when equilibrium is reestablished? A. [CH3COO-] and pH have both increased. B. [CH3COOH] and pH have both decreased. C. [CH3COO-] has decreased and pH remains relatively constant. D. [CH3COOH] has decreased and pH remains relatively constant. E. [CH3COO-] has increased and pH remains relatively constant.
Chemistry
1 answer:
Mila [183]3 years ago
6 0

Answer:

e

Explanation:

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3 years ago
If the molar heat of combustion of liquid benzene at constant volume and 300k is -3272KJ. Calculate the heat of combustion at co
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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)

\Delta n_g = (12 - 15)/2 = -3/2

We have;

\Delta H = \Delta U + \Delta n_g\cdot R\cdot T

Where R and T are constant, and ΔU is given we can write the relationship as follows;

H = U + \Delta n_g\cdot R\cdot T

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H = The heat at constant pressure

U = The heat at constant volume = -3,272 kJ

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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.

4 0
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