Question

Given the following information

A + B --> 2D delta H =684.9kJ delta S= 298.0J/K

C --> D delta H= 503.0kJ delta S=-103.0J/K

calculate ΔG° for the following reaction at 298 K.

A + B --> 2C

Answer #1

Lets number the reaction as 1, 2, 3 from top to bottom

required reaction should be written in terms of other reaction

This is Hess Law

required reaction can be written as:

reaction 3 = +1 * (reaction 1) -2 * (reaction 2)

So, deltaHo rxn for required reaction will be:

deltaHo rxn = +1 * deltaHo rxn(reaction 1) -2 * deltaHo rxn(reaction 2)

= +1 * (684.9) -2 * (503.0)

= -321.1 KJ

deltaSo rxn for required reaction will be:

deltaSo rxn = +1 * deltaSo rxn(reaction 1) -2 * deltaSo rxn(reaction 2)

= +1 * (298.0) -2 * (103.0)

= 92.0 J/K

deltaHo = -321.1 KJ

deltaSo = 92 J/K

= 0.092 KJ/K

T = 298 K

we have below equation to be used:

deltaGo = deltaHo - T*deltaSo

deltaGo = -321.1 - 298.0 * 0.092

deltaGo = -348.5 KJ

Answer: -348.5 KJ

given the following information
A+B->2D delta H=-710.9kJ delta S= 298.0J/K
C->D delta H =515kJ delta S=-192
J/K
calculate the delta G for the following reaction at 298K.
A+B->2C
**PLEASE SHOW WORK**

Consider the following reaction at 298 K:
2C (graphite) + O2 (g) >>> 2CO (g) Delta H = -221.0
kJ
Calculate: Delta S(sys) J/K Delta S (surr) J/K Delta S (Univ)
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Given the following information A+B⟶2DΔ?∘=750.7 kJΔ?∘=380.0 J/K
C⟶DΔ?∘=450.0 kJΔ?∘=−109.0 J/K calculate Δ?∘ at 298 K for the
reaction A + B --> 2C

HgO(s)
Hg(g)
O2(g)
Enthaply Delta H kj/mol
-90.8
61.3
Entropy Delta S j/mol. K
70.3
174.9
205.0
Above is a table of thermodynamics date for the chemical species
in the reaction: 2HgO(s) ----> 2Hg(g)+ O2(g) at 25 C
A) Calculate the molar entropy of reaction at 25 C
B) Calculate the standard Gibbs free enregy of the reaction at
25 C given that the enthaply of reaction at 25 C is 304.2
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C)Calculate the equilibrium constant for the reaction...

5. For a given reaction Delta H Standard = -45 kJ and Delta S
Standard = -103 J/K.
A. Is the reaction spontaneous? At what T does it become
spontaneous?
B. What is Delta G at 450 K?

Part A
Calculate the standard enthalpy change for the reaction
2A+B⇌2C+2D
where the heats of formation are given in the following
table:
Substance
ΔH∘f
(kJ/mol)
A
-227
B
-399
C
213
D
-503
Express your answer in kilojoules.
Answer= 273kJ
Part B:
For the reaction given in Part A, how much heat is absorbed when
3.70 mol of A reacts?
Express your answer numerically in kilojoules.
Part C:
For the reaction given in Part A, ΔS∘rxn is 25.0 J/K ....

4. Thermodynamic data for C(graphite) and
C(diamond) at 298 K is given in the table
below.
delta Hfo (kJ/mol)
o (J/mol K
C(graphite)
0.0
5.740
C(diamond)
1.895
2.377
a) Calculate delta Ho and delta So and
delta Go for the transformation of 1 mole of graphite
to diamond at 298 K.
b) Is there a tempature at which this transformation will occur
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a. delta H = 293 kj delta S = -695 J/K
b. delta H = -1137 kJ; delta S = 0.496 kJ/K
c. delta H = -86.6 kJ; delta S = -382 J/K

Calculate the delta H degrees reaction for the following
reaction:
2Ni(s) + 2S(s) +3O2 (g) -> 2NiSO3(s)
from the following info:
NiSO3(s) -> NiO(s) + SO2(g) delta H=156kJ
S(s) + O2(g) -> SO2(g) delta H= -297
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Calculate delta H for C+ 1/2 O2 --> CO
given:
C+ O2, delta H = -22kj
CO + 1/2 O2 --> Co2, delta H = -15kj

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