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 -241 B -391 C 197 D -497 Express
your answer in kilojoules. Hints ΔH∘rxn = 273 kJ SubmitMy
AnswersGive Up Correct Part B For the reaction given in Part A, how
much heat is absorbed when 2.80 mol of A reacts? Express your
answer numerically in kilojoules. Hints kJ SubmitMy AnswersGive Up
Part C...
Use data in Appendix C in the textbook to calculate ΔH∘ in
(kJ/mol) , ΔS∘ in (j/mol-K) , and ΔG∘ in (kJ/mol) at 25 ∘C for each
of the following reactions: 2P(g)+10HF(g)→2PF5(g)+5H2(g)
Appendix C:
P(g): dH:316.4; dG: 280.0; S:163.2
HF(g): dH: -268.61; dG: -270.70; S:173.51
PF5(g): dH:-1594.4; dG: -1520.7; S: 300.8
H2(g): dH:217.94; dG: 203.26; S: 114.60
For the reaction
A(aq) ---> B(aq)
the change in the standard free enthalpy is 2.59 kJ at 25
oC and 4.73 kJ at 45 oC. Calculate the value
of this reaction's equilibrium constant at 75 oC.
A scientist measures the standard enthalpy change for the following
reaction to be -613.2 kJ :
P4O10(s) + 6
H2O(l)-->4H3PO4(aq)
Based on this value and the standard enthalpies of formation for
the other substances, the standard enthalpy of formation of
H3PO4(aq) is kJ/mol.
a) The standard enthalpy change for the following reaction is
-270 kJ at 298 K.
2HCN (g) --> 2 C(s, graphite) + H2 (g) + N2 (g)
ΔH° = -270 kJ
What is the standard enthalpy change for this reaction at 298
K?
C (s, graphite) + 1/2 H2(g) + 1/2 N2(g) ---> HCN(g)
_______ kJ
A reaction
A + B <==> C
has a standard free-energy change of -3.27 kJ/mol at
25oC
What are the concentrations of A, B, and C at equilibrium if at the
beginning of the reaction their concentrations are 0.30M, 0.40M and
0M respectively?
Consider a gas phase reaction, 2A+B −↽−⇀− 3C+2D. When 1.00 mol A
and 2.00 mol B, and 1.00 mol D were mixed and allowed to come to
equilibrium at 25◦ C and ptotal = 1.0 bar, the resulting mixture
contained 0.90 mol C. Calculate (a)partial pressures of each at
equilibrium, (b) Keq, and (c) ∆rG.
A.) The standard enthalpy change for the following reaction is
359 kJ at 298 K.
PbCl2(s) ----> Pb(s) +
Cl2(g) ΔH° = 359
kJ
What is the standard enthalpy change for this reaction at 298
K?
Pb(s)
+ Cl2(g) ---->
PbCl2(s)
__________ kJ
B.) The standard enthalpy change for the following reaction is
-602 kJ at 298 K.
Mg(s)
+ 1/2 O2(g)
----> MgO(s) ΔH° =
-602 kJ
What is the standard enthalpy change for the reaction at 298
K?
2...