Question

Estimate the value of the equilibrium constant at 530 K for each of the following reactions. 2H2S(g)⇌2H2(g)+S2(g)

Answer #1

2H2S(g) <--------------> 2 H2 (g) + S2 (g)

ΔH∘rxn = ΔH∘f products - ΔH∘f reactants

= 129 - (2 x - 20.6)

= 170.2 kJ/mol

ΔSorxn = 2 x 130.7 + 228.1 - (2 x 205.7)

= 78.1 J/K

ΔGo = ΔH∘ - T ΔSo

= 170.2 - 530 x (- 0.0781)

= 211.6 kJ/mol

ΔGo = - RT ln K

211.6 = - 8.314 x 10^-3 x 530 x ln K

K = 1.40 x 10^-21

**Equilibrium constant K = 1.40 x 10^-21**

Estimate the value of the equilibrium constant at 550 K for each
of the following reactions.
a) 2CO(g)+O2(g)⇌2CO2(g)
b) 2H2S(g)⇌2H2(g)+S2(g)

Estimate the value of the equilibrium constant at 525 K for each
of the following reactions.
A.
2CO(g)+O2(g)⇌2CO2(g)
B.
2H2S(g)⇌2H2(g)+S2(g)

Estimate the value of the equilibrium constant at 525 K for each
of the following reactions.
A. 2CO(g)+O2(g)⇌2CO2(g)
B. 2H2S(g)⇌2H2(g)+S2(g)

Estimate the value of the equilibrium constant at 625 K for each
of the following reactions. ΔH∘f and S∘ for BrCl(g) is 14.6 kJ/mol
and 240.0 Jmol⋅K, respectively. Part A 2NO2(g)⇌N2O4(g) Please be
fast because it will soon be over by 11:59pm. Thank you

Consider the following reaction at equilibrium:
2H2(g)+S2(g)⇌2H2S(g)+heat
In a 10.0-L container, an equilibrium mixture contains 2.20 g of
H2, 10.9 g of S2 and 68.1 g of H2S.
Part A What is the numerical Kc value for this
equilibrium mixture?
Part B If more H2 is added to the equlibrium mixture, how will
the equilibrium shift?
Part C How will the equilibrium shift if the mixture is placed
in a 5.00-L container with no change in temperature?
Part D If...

A mixture of 1.00 g H2 and 1.06 g H2S in a 0.500−L flask comes
to equilibrium at 1670 K: 2H2(g)+S2(g)⇌2H2S. The equilibrium amount
of S2(g) found is 8.00×10−6mol. Determine the value of KP at 1670
K.

At 800 K, the equilibrium constant, Kp, for the following
reaction is 3.2 × 10–7 . 2 H2S(g) 2 H2(g) + S2(g) A reaction vessel
at 800 K initially contains 3.00 atm of H2S. If the reaction is
allowed to equilibrate, what is the equilibrium pressure of S2?

The equilibrium constant is given for two of the reactions
below. Determine the value of the missing equilibrium constant.
2A(g) + B(g) ⇌ A2B(g) Kc = ? A2B(g) + B(g) ⇌ A2B2(g) Kc = 16.4
2A(g) + 2B(g) ⇌ A2B2(g) Kc = 28.2

Use data from Appendix IVB to calculate the equilibrium
constants at 25∘C for each reaction. Express your answer using two
significant figures.
Part A: 2CO(g)+O2(g)⇌2CO2(g)
Part B: 2H2S(g)⇌2H2(g)+S2(g)

For chemical reactions involving ideal gases, the equilibrium
constant K can be expressed either in terms of the concentrations
of the gases (in M) or as a function of the partial pressures of
the gases (in atmospheres). In the latter case, the equilibrium
constant is denoted as Kp to distinguish it from the
concentration-based equilibrium constant K.
Part A
For the reaction
2CH4(g)⇌C2H2(g)+3H2(g)
K = 0.155 at 1635 ∘C . What is Kp for the
reaction at this temperature?
Express...

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