Question

H2(g) + C2H4(g)C2H6(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K.

Answer #1

1. NH4Cl(aq)<->NH3(g) + HCl(aq)
Using the standard thermodynamic data in the tables linked
above, calculate the equilibrium constant for this reaction at
298.15K.
2. HCl(g) +
NH3(g)NH4Cl(s)
Using the standard thermodynamic data in the tables linked above,
calculate the equilibrium constant for this reaction at
298.15K.

Consider the reaction 2H2O2(l)2H2O(l) + O2(g) Using the standard
thermodynamic data in the tables linked above, calculate the
equilibrium constant for this reaction at 298.15K.

Consider the reaction
N2(g) +
2O2(g)----->2NO2(g)
Using the standard thermodynamic data in the tables linked above,
calculate Grxn for this reaction at 298.15K if the
pressure of each gas is 29.25 mm Hg.
Consider the reaction
4HCl(g) +
O2(g)------>2H2O(g)
+ 2Cl2(g)
Using the standard thermodynamic data in the tables linked above,
calculate G for this reaction at 298.15K if the pressure of each
gas is 12.40 mm Hg.

Consider the reaction 2CO2(g) + 5H2(g)C2H2(g) + 4H2O(g) Using
the standard thermodynamic data in the tables linked above,
calculate G for this reaction at 298.15K if the pressure of each
gas is 17.64 mm Hg.
ANSWER:_____ kJ/mol

1)Use standard thermodynamic data (in the Chemistry References)
to calculate G at 298.15 K for the following reaction, assuming
that all gases have a pressure of 19.31 mm Hg. 2N2(g) +
O2(g)2N2O(g)
G = ? kJ/mol
2)Using standard thermodynamic data (linked), calculate the
equilibrium constant at 298.15 K for the following reaction.
C2H4(g) + H2O(g)CH3CH2OH(g)
K = ?
3) Calculate the temperature (in kelvins) at which the sign of
G° changes from positive to negative for the reaction below. This...

4) Let’s combine multiple equilibrium.
C2H6(g) <--> C2H4(g) + H2(g) kp = 2.8x10-10
N2(g) + 3 H2(g) <--> 2NH3(g) kp = 1.64x10-4
If C2H6 = 10atm, N2 = 10atm and H2 = 50atm
find the concentrations at equilibrium.

Use the standard reduction potentials located in the 'Tables'
linked above to calculate the equilibrium constant for the
reaction: Co2+(aq) + 2Cu+(aq) Co(s) + 2Cu2+(aq) Hint: Carry at
least 5 significant figures during intermediate calculations to
avoid round off error when taking the antilogarithm. You may use
the OWL references to find the values you may need in this
question. Equilibrium constant: G° for this reaction would be than
zero.

Calculate the ΔH∘ for this reaction using the following
thermochemical data:
CH4(g)+2O2(g)⟶CO2(g)+2H2O(l)
ΔH∘=−890.3kJ
C2H4(g)+H2(g)⟶C2H6(g)
ΔH∘=−136.3kJ
2H2(g)+O2(g)⟶2H2O(l)
ΔH∘=−571.6kJ
2C2H6(g)+7O2(g)⟶4CO2(g)+6H2O(l)

Estimate the rate constant for the reaction H2 + C2H4 ? C2H6 at
628 K knowing that the calculated reduced mass, using m(H2) =
2.016mu and m(C2H4) = 28.05mu, is ? = 3.123 × 10?27 kg, ?(H2,C2H4)
? 0.44 nm2 , and the activation energy is 180 kJ mol?1

Given the standard reaction enthalpies for these two
reactions:
(1) 2C(s) + 2H2(g) = C2H4(g)...... ΔrH° = 52.3 kJ/mol
(2) 2C(s) + 3H2(g) = C2H6(g)......ΔrH° = -84.7 kJ/mol
calculate the standard reaction enthalpy for the reaction: (3)
C2H4(g) + H2(g) = C2H6(g)......ΔrH° = ?

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