The bisulfate (or hydrogen sulfate) anion, HSO 4 − , is a weak acid. The equilibrium constant for the aqueous acid reaction HSO 4 − ( aq ) ⇌ H + ( aq ) + SO 4 2 − ( aq ) is 1.2 × 10 − 2 . (a ) Calculate Δ G ° for this equilibrium. Assume a temperature of 25.0 ° C . (b) At low concentrations, activity coefficients are approximately 1 and the activity of a dissolved solute equals its molality. Determine the equilibrium molalities of a 0.010 -molal solution of sodium hydrogen sulfate.
The bisulfate (or hydrogen sulfate) anion, HSO 4 − , is a weak acid. The equilibrium constant for the aqueous acid reaction HSO 4 − ( aq ) ⇌ H + ( aq ) + SO 4 2 − ( aq ) is 1.2 × 10 − 2 . (a ) Calculate Δ G ° for this equilibrium. Assume a temperature of 25.0 ° C . (b) At low concentrations, activity coefficients are approximately 1 and the activity of a dissolved solute equals its molality. Determine the equilibrium molalities of a 0.010 -molal solution of sodium hydrogen sulfate.
The bisulfate (or hydrogen sulfate) anion,
HSO
4
−
, is a weak acid. The equilibrium constant for the aqueous acid reaction
HSO
4
−
(
aq
)
⇌
H
+
(
aq
)
+
SO
4
2
−
(
aq
)
is
1.2
×
10
−
2
.
(a) Calculate
Δ
G
°
for this equilibrium. Assume a temperature of
25.0
°
C
.
(b) At low concentrations, activity coefficients are approximately
1
and the activity of a dissolved solute equals its molality. Determine the equilibrium molalities of a
0.010
-molal solution of sodium hydrogen sulfate.
Assuming that neither standard enthalpy changes of formations (∆Hof) nor standard molar entropies (So) depend upon temperature, estimate using the Table of Thermodynamic Data : (a) the standard Gibbs free energy change for the reaction that forms rhombic sulfur at 600 K, and (b) the temperature (in oC) at which reaction will stop formation of products:
2H2S(g) + SO2(g) → 3S(rhombic, s) + 2H2O(g)
Round off your answers to the nearest integer. Report the temperature in oC. and enter them with correct units:
(a)∆Gorxn =
(b) T =
Consider the reactions in the table.
(a) Write the equilibrium constant in terms of activities for the chemical reaction of fire extinguishers: 2NaHCO3 (s) ↔ Na2CO3 (s) + CO2 (g) + H2O (g) ΔrH = 135.54 KJ
(b) At 300 K the equilibrium constant is 3.95x10-6 for the reaction in (a), what is ΔrGo?
(c) State in words: what happens to the equilibrium when temperature is increased? Then, verify by finding K for the reaction in (a) at 420 K.
Consider the following reaction at 100.0 °C:
Al(s) + NaOH(aq) + H20(l) ⇄ Na[Al(OH)4](aq) + H2(g)
A) Write a balanced equilibrium quotient (Qc) for the following reaction.
B) If the pressure of this reaction is increased, which direction will the equilibrium shift? Why?
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The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY