Phosphorus and bromine react to form phosphorus tribromide, like this: P4(9)+6 Br,(g)→4 PBr;(g) Write the pressure equilibrium constant expression for this reaction.

Predict the equilibrium concentration of NH in the reaction described below (for which Kc = 1.210 at the reaction temperature) by constructing an ICE table, writing the equilibrium constant expression, and solving for the equilibrium concentration. Complete Parts 1-3 before submitting your answer. = NHSH(s) NH¸(g) + H₂S(g) Using the data from your ICE Table (Part 1), construct the expression for the equilibrium constant, Kc. Each reaction participant must be represented by one tile. Do not combine terms. KC = II = 1.2 × 10-4 RESET [x] [2x] [2x]² [1.2 × 104+x] [1.2 × 104-x] [1.2 × 104 + 2x] [1.2 × 104 -2x] [1.2 × 10+ + x]² [1.2 × 10+ - x]² [1.2 × 10+ + 2x]² [1.2 × 104 -2x]²

Consider the reaction: N2(g) + 3H2(g) 2NH3(g) where Kc = 0.500 at 400 °C. If 50.0 L reaction vessel contains 1.000 mole N₂; 3.000 mole H₂ and 0.050 mole NH3, which of the following is TRUE? The reaction based on the following parameters is in equilibrium. More ammonia will be produced as the reaction approaches equilibrium. Data provided is not enough to warrant a conclusion regarding equilibrium. More ammonia will dissociate as the reaction approaches equilibrium.

The equilibrium constant for the chemical equation N,(g) + 3 H, (g) 2 NH,(g) is K, 0.356 at 197 °C. Calculate the value of the K, for the reaction at 197 °C. K.

The equilibrium constant for the chemical equation N,(g) + 3 H, (g) = 2 NH, (g) is Kp = 0.402 at 267 °C. Calculate the value of K. for the reaction at 267 °C. K. =

Most reaction do not go to completions. Equilibrium is established between the reactants and products. For the reaction of A with B to produce C and D, we can write the chemical equation as: аА + bв + сс + dD where + represents equilibrium between the reactants and products. The extent to which the reaction proceeds to product formation, at a given temperature, is given by the equilibrium constant, Kę. The equilibrium constant is written mathematically (for the above equation) as: [C[[D]* K. = [A]°[B]" where, a, b, c, and d are the stoichiometric coefficients from the balanced chemical equation and the brackets, [ ], indicate molar concentration. 1. For the following reaction: 2A + В + 3с calculate the equilibrium constant, K, if at equilibrium the concentration of A is 0.15M, the concentration of B is 0.20M, and the concentration of C is 0.10M.

The equilibrium constant for the synthesis of ammonia N2(g) + 3 H2(g) --> 2 NH3(g) has the value K = 3.19 × 10^-4 at  400°C. Calculate the equilibrium partial pressures of N2(g), H2(g), and NH3(g) if the total pressure is 1.00 atm and the H:N atomratio in the system is 3;1. (Hint: Try the approximationthat PN2  and PH2  > PNH3  and see if the resulting equationsare simpliied.)

Write the pressure equilibrium constant expression for this reaction. 2 CO,(g)+4 H,O(g)→2CH;OH(1)+3 O2(9)

Write the equilibrium expression, in terms of pressure, for the formation of ammonia equilibrium.

(a) What does it mean when the reaction quotient, Q, is numerically equal to the equilibrium constant, Kc? (b) What does it mean when it is less than the equilibrium constant? (c) What does it mean when it is less than the equilibrium constant?