a) 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 0.251 moles
ofCH4and 0.251 moles
of CCl4are introduced into a 1.00 L
vessel at 350 K.
[ CH4] | = | M |
[ CCl4] | = | M |
[ CH2Cl2] | = | M |
b) The equilibrium constant, Kc, for the following
reaction is 1.20×10-2 at
500 K.
PCl5(g)
->PCl3(g) +
Cl2(g)
Calculate the equilibrium concentrations of reactant and products
when 0.223 moles of
PCl5(g) are introduced into a 1.00 L
vessel at 500 K.
[PCl5] | = | M |
[PCl3] | = | M |
[Cl2] | = | M |
C) The equilibrium constant, Kc, for the following
reaction is 10.5 at 350 K.
2CH2Cl2(g)
->CH4(g) +
CCl4(g)
Calculate the equilibrium concentrations of reactant and products
when 0.313 moles of
CH2Cl2 are introduced into a
1.00 L vessel at 350 K.
[CH2Cl2] | = | M |
[CH4] | = | M |
[CCl4] | = | M |
a) The equilibrium constant, Kc, for the following reaction is 9.52×10-2at 350 K. CH4(g) + CCl4(g)...
The equilibrium constant, Kc, for the following reaction is 9.52×10-2 at 350 K: CH4(g) + CCl4(g) <---> 2CH2Cl2(g) Calculate the equilibrium concentrations of reactants and product when 0.343 moles of CH4 and 0.343 moles of CCl4 are introduced into a 1.00 L vessel at 350 K. [CH4] = M [CCl4] = M [CH2Cl2] = M
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The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCl3(g) + Cl2(g) ⇌ PCl5(g) Calculate the equilibrium concentrations of reactant and products when 0.253 moles of PCl3 and 0.253 moles of Cl2 are introduced into a 1.00 L vessel at 500 K. [PCl3] = ___ M [Cl2] = ___ M [PCl5] = ___M
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