Given the following information:
energy of sublimation of Li( s)= 166 kilojoules per mole
find bond energy of HCL= 427 kilojoules per mole
ionization energy of Li(g) =520 kilojoules per mole
electron affinity of Cl(g) =-349 kilojoules per mole
lattice energy of LiCl(s)=-829 kilojoules per mole
bond energy of H2= 432 kilojoules per mole
calculate the net change in energy for the following
reaction:
2Li(s)+2HCl(g)------->2LiCl(s) + H2(g)
Cd (s) + NiO(OH) (s) -> Cd(OH)2 (s) + Ni(OH)2 (not
balanced)
a. Balance the reaction above usingt the 1/2 reaction method, in
alkaline conditions
b.`if 5.00 g of Cd and 7.5 g of NiO(OH) are combined, which will
be the limiting reactant? How much of the other reactant will
remain after the reaction completes?
Calculate the maximum amount of work for the redox reaction
between Cd(s) and Au^3+(aq) at 25 ̊C
Answer = 1.10 x 10^6 J
Can anyone please work this out?
Calculate enthalpy for the following reaction Ca(s) + 1/2O2 +
CO2 = CaCo3 Given the following reactions: Ca(s) + 1/2 O2 = CaO (s)
H= -635.1 kj CaCo3 = CaO (s) + CO2 H= 178.3 kj
(a) Calculate the standard free-energy change (ΔG°) for the
following oxidation-reduction reaction. Cu(s) + Br2(aq) → Cu2+(aq)
+ 2 Br−(aq)
(b) Calculate the equilibrium constant for this reaction at 298
K.
Calculate the standard change in Gibbs free energy, ΔGrxn∘, for
the given reaction at 25.0 ∘C. Consult the table of thermodynamic
properties for standard Gibbs free energy of formation values.
KBr(s)↽−−⇀K+(aq)+Br−(aq)
ΔGrxn°= ? kJ/mol
Determine the concentration of K+(aq) if the change in Gibbs
free energy, nΔGrxn, for the reaction is −8.95 kJ/mol.
[K+] = ? M
You are given the following information for a closed economy in
a general equilibirum context.
Cd = 5000 + 0.8Y - 80,000r
, Id = 1000 - 45,000r.
Md/P = 0.9Y - 4000i
, π e = 0.05, G = 450,
Y-bar= 1000, and M = 3000.
a) Calculate the general equilibrium values of the real interest
rate and the price level.
b) Explain what general equilibrium means in the IS-LM framework
and how it is attained.
c) What kind of...