2HI -> H2 + 12 K = 3.2 x 10 - 16 If the initial concentration of HI is 0.2 mol/L, determine the concentrations of all entities at equilibrium.

Consider the reaction: 2 HI (g) = H2 (g) + 12 (g) Kc = 7.21 If at equilibrium the reaction vessel contains 1.20 M of H₂ and 1.70 M then what is the equilibrium concentration of HI? 2⁹ 1 4 7 2 DO 8 +/- 5 M 3 6 9 00 0 X с x 100 +

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At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H₂(g) + 1₂(g) 2 HI(g) Kc = 53.3 At this temperature, 0.300 mol H₂ and 0.300 mol I₂ were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium?

Write the pressure equilibrium constant expression for this reaction.  2CH3OH(l)+3Os(g) --> 2CO2(g)+4H2O(g)

Payalben

2. A mixture of 0.500 mol Nz and 0.500 mol H2 was placed in a 1.00-L stainless-steel flask at 430 degrees Celsius. Determine the value of the equilibrium constant, Kc, when the equilibrium concentration of nitrogen [N2] (g) = 0.43 M. N2 (g) + 3H2 (g) -> 2NH3 (g)

[References] The equilibrium constant (K) for the reaction PCI3 (g) + Cl2 (g) PCl; (g) equals 49 at 230°C. If 0.378 mol each of phosphorus trichloride and chlorine are added to a 6.30 L reaction vessel, what is the equilibrium composition of the mixture at 230°C? mol PC13 mol Cl2 mol PCI5

At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, Kc, which is a mathematical expression based on the chemical equation. For example, in the reaction aA+bB⇌cC+dD where a, b, c, & d are the stoichiometric coefficients, the equilibrium constant is Kc=[C]c[D]d[A]a[B]b & where [A][A], [B][B], [C][C], and [D][D] are the equilibrium concentrations. If the reaction is not at equilibrium, the quantity can still be calculated, but it is called the reaction quotient, Qc, instead of the equilibrium constant, Kc.Qc=[C]tc[D]td[A]ta[B]tb where each concentration is measured at some arbitrary time t. Part A  A mixture initially contains AA, BB, and CC in the following concentrations: [A]= 0.700 M, [B]= 1.40 M, & [C]= 0.550 M. The following reaction occurs and equilibrium is established: A+2B⇌CA+2B⇌C At equilibrium, [A]= 0.520 M & [C]= 0.730 M. Calculate the value of the equilibrium constant, Kc.

Write the equilibrium constant expression, Kc, for the equation:                         2NO2(g)  +  7H2(g)   -----> 2NH3(g)  +  4H2O(g) Write the equilibrium constant expression, Kc, for the reverse of the previous reaction.