The following reaction was performed in a sealed vessel at 775 ∘C∘C : H2(g)+I2(g)⇌2HI(g)H2(g)+I2(g)⇌2HI(g) Initially, only H2H2 and I2I2 were present at concentrations of [H2]=3.25M[H2]=3.25M and  [I2]=2.20M[I2]=2.20M . The equilibrium concentration of I2I2 is 0.0200 MM . What is the equilibrium constant, KcKcK_c, for the reaction at this temperature?

The equilibrium constant, Kc, for the following reaction is 1.29x10-2 at 600 K. coCI,(g) ? CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.373 moles of COCI2(g) are introduced into a 1.00 L vessel at 600 K. [COCI2] = [CO] M [Cl2] M ΣΣΣ

The equilibrium constant for the reaction 2 HF (g) ⇌ H₂ (g) + F₂ (g) is 0.300 at a particular temperature. What is the equilibrium constant for the equation ½ H₂ (g) + ½ F₂ (g) ⇌ HF (g)?

For the reaction N2(g)+3H2(g)⇌2NH3(g)N2(g)+3H2(g)⇌2NH3(g) KpKpK_p = 4.25×10−3 at 334 ∘C∘C . What is KcKc for the reaction at this temperature? Enter your answer numerically.

As shown in Table 15.2 in the textbook, KpKp for the equilibriumN2(g)+3H2(g)⇌2NH3(g)N2(g)+3H2(g)⇌2NH3(g)is 4.51×10−54.51×10−5 at 450 ∘C∘C. For each of the mixtures listed here, indicate whether the mixture is at equilibrium at 450 ∘C∘C. If it is not at equilibrium, indicate the direction (toward product or toward reactants) in which the mixture must shift to achieve equilibrium. A. 98 atmatm NH3NH3, 45 atmatm N2N2, 55 atmatm H2H2 98  , 45  , 55   a. yes, mixture is at equilibrium b. no, mixture must shift toward products to achieve equilibrium c. no, mixture must shift toward reactants to achieve equilibrium B.57 atmatm NH3NH3, 143 atmatm N2N2, no H2H2 57  , 143  , no  a.yes, mixture is at equilibrium b.no, mixture must shift toward products to achieve equilibrium c.no, mixture must shift toward reactants to achieve equilibrium

For the reaction 2A(g)⇌B(g)+2C(g)2A(g)⇌B(g)+2C(g), a reaction vessel initially contains only A at a pressure of PA=245 mmHgPA=245 mmHg . At equilibrium, PA=71 mmHgPA=71 mmHg .     Part A Calculate the value of KpKp. (Assume no changes in volume or temperature.)         Express your answer using two significant figures.

For the following reaction: NH4Cl(s) ↔ NH3(g) + HCl(g) ΔH = +42.1 kilocalories Suppose the substances in the reaction above are at equilibrium at 600K in volume V and at pressure P. State whether the partial pressure of NH3(g) will have increased, decreased, or remained the same when equilibrium is reestablished after each of the following disturbances of the original system. Some solid NH4Cl remains in the flask at all times. Justify each answer with a one-or-two sentence explanation. (e) A quantity of gaseous NH3 is added. The answer for e states that the partial pressure of NH3 is increase, which is a bit confusing. The explanation is that some of the the added NH3 reacts with HCl to relieve stress but only part of NH3 reacts. Can you explain how and where this is implied in the reaction or question. Would appreciate a lot of clarification

The following reaction was carried out in a 4.00 LL reaction vessel at 1100 KK: C(s)+H2O(g)⇌CO(g)+H2(g)C(s)+H2O(g)⇌CO(g)+H2(g) If during the course of the reaction, the vessel is found to contain 7.25 molmol of CC, 15.5 molmol of H2OH2O, 3.80 molmol of COCO, and 6.10 molmol of H2H2, what is the reaction quotient QQQ? Enter the reaction quotient numerically.

Calculate the equilibrium concentrations of  N2O4  and  NO2  at 25  ∘C  in a vessel that contains an initial  N2O4  concentration of 0.0538  M  . The equilibrium constant  Kc  for the reaction  N2O4(g)⇌2NO2(g)  is  4.64×10−3  at 25  ∘C .Express your answers using four decimal places separated by a comma.

Write the expression for the equilibrium constant Kp for the following reaction.Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH3)2 as (P NH3)2 . If either the numerator or denominator is 1, please enter 1   2 Co3O4(s)   ↔   6 CoO(s) + O2(g)