The equilibrum constant Kc is 0.01323 for the reaction: CCl4 (g)
<----> C(s) + 2 Cl2 (g)
At 300k a 5L flask originally contained 0.0828M of CCl4, 0.0444
M of C and 0.0546M of Cl2. Determine the concentration of Cl2 when
equilibrium is reached.
1. The equilibrium constant, Kc, for the following
reaction is 9.52×10-2at
350 K.
CH4(g) +
CCl4(g) = 2
CH2Cl2(g)
Calculate the equilibrium concentrations of reactants and product
when 0.300 moles of
CH4and 0.300 moles of
CCl4are introduced into a 1.00 L vessel
at 350 K.
[ CH4]
=
M
[ CCl4]
=
M
[ CH2Cl2]
=
M
2. 2HI(g)
=H2(g) +
I2(g)
If 1.87 moles of HI,
0.335 moles of H2, and
0.211 moles of I2 are
at equilibrium in...
The equilibrium constant KP for CCl4(g) f15g2a33g1.jpgC(s) + 2
Cl2(g) is 0.76 at 700 K. What percentage (%) of CCl4 is converted
into C and Cl2 when a flask charged with 3.00 atm of CCl4 reaches
equilibrium at 700 K?
Calculate ΔrH for the following reaction:
CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g)
Use the following reactions and given ΔrH's.
C(s)+2H2(g)→CH4(g)ΔrH=−74.6kJmol−1C(s)+2Cl2(g)→CCl4(g)ΔrH=−95.7kJmol−1H2(g)+Cl2(g)→2HCl(g)ΔrH=−92.3kJmol−1
Calculate ΔrH for the following reaction:
CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g)
Use the following reactions and given ΔrH's.
C(s)+2H2(g)→CH4(g)ΔrH=−74.6kJmol−1C(s)+2Cl2(g)→CCl4(g)ΔrH=−95.7kJmol−1H2(g)+Cl2(g)→2HCl(g)ΔrH=−92.3kJmol−1
At 100.0 C, the equilibrium constant for the reaction: CO (g) +
Cl2 (g) <--> COCl2 (g) has a value of
4.6 x 109. If 0.40 mol of COCl2 is placed
into a 10.0 L flask at 100.0 C, what will be the equilibrium
concentration of all species? (A simplifying approximation that
will make the solution of the resulting equation easier is to note
that x is much less than 0.040mol/L. This means that 0.040 -x is
approximately 0.040.)
(a) For the reaction 2 A(aq) ⇋ 2 B(g) + C(g), the equilibrium
constant is 4.59 at 25.0oC. If the concentrations of B(aq) and
C(aq) are each 0.311 M, what concentration of A(aq) is required to
have a ΔG value of -6.66 kJ/mol? The temperature is 25.0oC.
(b) We have a buffer solution that was produced by adding 11.9 g
of NaOH to 2.000 L of a 0.666 M solution of HA(aq). The pH of the
buffer solution is 3.25...