Question

When the oxide of generic metal M is heated at 25.0 °C, only a negligible amount of M is produced. reaction

MO(s) <-> M(s) + O2.

delta G is 287.8 kj/ mol. When this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous.

What is the chemical equation of this coupled process? Show that the reaction is in equilibrium, include physical states, and represent graphite as C(s). ??

Answer #1

When the oxide of generic metal M is heated at 25.0 °C, only a
negligible amount of M is produced.
MO2(s) <-> M(s) + O2(g) Deltra G = 287.3 kJ/mol
When this reaction is coupled to the conversion of graphite to
carbon dioxide, it becomes spontaneous.
What is the chemical equation of this coupled process? Show that
the reaction is in equilibrium, include physical states, and
represent graphite as C(s).
What is the thermodynamic equilibrium constant for the coupled
reaction?...

Consider the decomposition of a metal oxide to its elements
where M represents a generic metal:
M2O (s) ⇌ 2 M (s) + 1/2 O2 (g)
Substance: ----> ∆G°f (kg/mol): M2O(s)
----------->-7.00
M(s) --------------> 0
O2(g) --------------->0
1. What is the standard change in Gibbs energy for the reaction
as written in the forward direction? ∆G°rxn = ? kj/mol
2. What is the equilibrium constant for this reaction as written
in the forward direction at 298 K? K = ?...

Substance
ΔG°f(kJ/mol)
M3O4(s)
−8.80
M(s)
0
O2(g)
Consider the decomposition of a metal oxide to its elements,
where M represents a generic metal.
M3O4(s)↽−−⇀ 3M(s)+2O2(g)
What is the equilibrium constant of this reaction, as written,
in the forward direction at 298 K?
What is the equilibrium pressure of O2(g) over M(s)
at 298 K?

Consider the decomposition of a metal oxide to its elements,
where M represents a generic metal Find: -Grxn -K -P(o2)
M2O3(s)<----> 2M(s) +3/2O2 (g) M2O3= -6.70 M(s)=0 02=0 Please
explain

When heated, calcium carbonate (calcite) decomposes to form
calcium oxide and carbon dioxide gas
CaCO3(s) <----> CaO(s) + CO2(g)
Using the data below, calculate the equilibrium partial pressure of
CO2(g) over a mixture of solid CaO and CaCO3 at 500 ◦C if ∆CP,m for
the reaction is independent of temperature over the temperature
range between 25 ◦C and 500 ◦C
...............................CaO(s)..........CO2(g)..............
CaCO3(s)
∆H◦ f (kJ/mol) .......−635.09 ......−393.51
............−1206.92
S◦ m (J / mol K) ......39.75 .........213.74
.................92.90
CP,m (J /...

When heated, calcium carbonate decomposes to yield calcium oxide
and carbon dioxide gas via the reaction
CaCO3(s)→CaO(s)+CO2(g)
What is the mass of calcium carbonate needed to produce 77.0 L
of carbon dioxide at 1 bar and 273 K?
Express your answer with the appropriate units.

In a generic chemical reaction involving reactants A and B and
products C and D, aA+bB→cC+dD,
the standard enthalpy ΔrH∘ of the reaction is given by
ΔrH∘=cΔfH∘(C)+dΔfH∘(D)
−aΔfH∘(A)−bΔfH∘(B)
Notice that the stoichiometric coefficients, a,
b, c, d, are an important part of this
equation. This formula is often generalized as follows, where the
first sum on the right-hand side of the equation is a sum over the
products and the second sum is over the reactants:
ΔrH∘=∑productsnΔfH∘−∑reactantsmΔfH∘
where m and...

A metal reacts with concentrated hydrochloric acid (12 M HCl) to
give the soluble metal hexachloride based on the following
reaction:
M (s) + 6 HCl (aq) → MCl6 (aq) + 3 H2 (g)
If it takes 23 mL of concentrated hydrochloric acid to fully
dissolve 8.5 g of the metal, what is the identity of the metal?
Give the answer as the chemical symbol:
0.35 L of a P4 solution with a concentration of 0.70 M and 2.5 L...

In a generic chemical reaction involving reactants A and B and
products C and D, aA+bB→cC+dD, the standard enthalpy ΔH∘rxn of the
reaction is given by ΔH∘rxn=cΔH∘f(C)+dΔH∘f(D) −aΔH∘f(A)−bΔH∘f(B)
Notice that the stoichiometric coefficients, a, b, c, d, are an
important part of this equation. This formula is often generalized
as follows, where the first sum on the right-hand side of the
equation is a sum over the products and the second sum is over the
reactants: ΔH∘rxn=∑productsnΔH∘f−∑reactantsmΔH∘f where m and...

1) The free energy change for the following reaction at 25 °C,
when [Pb2+] = 1.18 M
and [Cd2+] =
7.90×10-3 M, is -65.9
kJ:
Pb2+(1.18 M) +
Cd(s)>
Pb(s) +
Cd2+(7.90×10-3
M) ΔG = -65.9 kJ
What is the cell potential for the reaction as written under these
conditions?
Answer: ___V
Would this reaction be spontaneous in the forward or the reverse
direction?
2) Use the standard reduction potentials located in the 'Tables'
linked above to calculate the standard...

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