3) The following are at constant T and P. The conditions described in (a) and (b)...
3) The following are at constant T and P. The conditions described in (a) and (b) below are initial conditions. Calculate Qc and CLEARLY indicate, with an arrow ("", or " to which side the reaction must shift in order to attain equilibrium. (a) A 250.0-ml flask containing 0.0250 mol of NO(g), 0.0100 mol of Cl2(g), and 0.250 mol of NOCI: 2NO(g) + Cl2(g) O 2NOCI(g) K= 4.6 x 10 (b) A 5.00-L flask containing 35.0 g of NH3, 20.0...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 bar for all species. For the reaction N2(g)+3H2(g)↽−−⇀2NH3(g) the standard change in Gibbs free energy is Δ?∘=−69.0 kJ/mol. What is Δ? for this reaction at 298 K when the partial pressures are ?N2=0.500 bar, ?H2=0.150 bar, and ?NH3=0.750 bar? Show work please!
Write the expressions for Kp for the following reactions: 1. a) 2NH3(g) + Co2(g) N2CH40(s) + H20 (I) b) CuO (s) + H2(g) Cu(l)+H20 (g) 2. At room temperature, a 1.5 L flask contains 3.0 moles of Cl, 0.5 mole of NOCI, and 4.0x10 mole of NO. Calculate Ke at this temperature for the following reaction: 2NO (g) + Cl2(g) 2NOCİ (g) 0.00245 M, does this represent a system at M, [No] 0.2 M and [Ch] If [NOCI] 2.0x 10...
pages 2-4 please! its equilibrium worksheet
2. A sample of gaseous BrCl is allowed to decompose in a closed container at 25C according to the equation below: 2BrCl(g) Bra(g) + Cl2(g) When the reaction reaches equilibrium, the following concentrations were obtained: [BrCl] = 0.38 M, [Cl:] = 0.26 M & [Br2] = 0.26 M. Determine the equilibrium constant for the reaction 3. A mixture of gases NOCI, Cl and NO was allowed to reach equilibrium at a particular temperature. The...
The general form of a chemical reaction is aA + bB = cC +dD Where A and B are reactants in the forward direction and C and D are products in the forward direction. The lower case letters are the stoichiometric coefficients for the balanced equation. The general form of the equilibrium constant equation is then: Keq = [C]c[D]d/[A]a[B]b Part I: Q vs. K Q: reaction quotient can be calculated for a reaction at any concentration values of reactants and...
pages 1-4 go together, and last question is separate but needs
an answer.
separate question: Which state of matter is the most
energetic? give a reason for your answer.
CHEM&121 WS-11: Equilibrium Worksheet 1. Write the equilibrium expression for the following reactions: a. 200+ 0 2CO b. COCl2 CO + Cl2 c. CS2 + 4H CH. +2H:S d. 2SO2 + 0 2SO e. 2C1:05 O2 + 4CIO 1 2. A sample of gaseous BrCl is allowed to decompose in a...
True or False
t. For an exothermic reaction, the equilibrium constant, Kc, becomes smaller as the temperature increases and larger as the temperature decreases. u. The gas-phase equilibrium shown below is used to produce ammonia, NH3, for commercial applications. The NH3 yield can be increased by decreasing the temperature, increasing the pressure, and removing some NH; from the mixture. N2(g) + 3H2(g) - 2NH3() AH = -94 kJ. v. For the gas-phase equilibrium described above (see problemlu), an increase in...
Which of the following expressions is the correct equilibrium-constant expression for the reaction below? 200(g) = CO2(g) + C(s) A. [CO][C]/[CO] B. K [CO] C. [CO] / [CO2) D. [CO]/[CO] E. 2[CO] /[CO][C] In which of the following reactions would increasing pressure at constant temperature not change the concentrations of reactants and products, based on Le Châtelier's principle? ООООО A. 2N, () + 0,02N,0 () B. N.O. (g) 2NO, (g) C. N2(g) + 3H2(g)2NH3 (9) D. N2 (9) + 202...
i need help with everything please!!
WWLWUNA HOSILNILNIUSPRING 2020) Chapter #14 The following practice problems from Chang's text are not to be submitted. The numbers in brackets refer to problems appearing at the end of the chapter. Equilibrium Constant Expressions (14.8, 14.9) Calculating Equilibrium Constants (14.13 to 14.24: Do as many as you can) Multiple Equilibria (14.29, 14.31) Kinetics and Chemical Equilibrium (14.35, 14.36) Calc. of Equilibrium Conc. (14.39 - 14.48) Do as many as you can. LeChatlier's Principle (14.54,...
2. The equilibrium constant for the dissociation of Ag,CO, (s) + 2 Ag+ + CO, is Kp -8.1 10-12 at 25°C. a) Calculate AG for the reaction when [Ag'] = 1.0 x 10 2M and CO, +1 = 1.0 x 10- M. (4pts) Ans: b) (Ipt) Is the reaction spontaneous or nonspontaneous at these concentrations? Ans: 3. (4pts) Nitrosyl chloride (NOCI) decomposes at elevated temperatures according to the equation below; 2NOCI(g) 2NO(g) + Cl2(g) Calculate K, for this reaction at...