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
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 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?
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...