Part A The reaction N2(g) + O2(9)=2NO(g) is carried out at a temperature at which K = 0.070. The reaction mixture starts with only the product, [NO]=0.0500 M, and no reactants. You may want to reference (Page) Section 15.8 while completing this problem. Find the equilibrium concentrations of N2 at equilibrium. Express your answer to two significant figures and include the appropr ? HÅ [N2]= Value Units Submit Request Answer Part B Find the equilibrium concentrations of O2 at equilibrium. Express your answer to two significant figures and include the appropri

Part A The reaction N2(g) + O2(9)=2NO(g) is carried out at a temperature at which K = 0.070. The reaction mixture starts with only the product, [NO]=0.0500 M, and no reactants. You may want to reference (Page) Section 15.8 while completing this problem. Find the equilibrium concentrations of N2 at equilibrium. Express your answer to two significant figures and include the appropr ? HÅ [N2]= Value Units Submit Request Answer Part B Find the equilibrium concentrations of O2 at equilibrium. Express your answer to two significant figures and include the appropri

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The equilibrium constant, Kc, for the following reaction is 2.0. If the equilibrium mixture contains 1.8 M NO and 0.70 M Br2, what is the molar concentration of NOBr? 2NOB1(g) = 2NO(g) +Br2 (g) Express your answer to two significant figures and include the appropriate units.
1. The diagrams below represent the following reversible chemical reaction: H2(g) + 12 (g) =2 HI (g) At 448 °C, the equilibrium constant, K, for this reaction is 51 Initial Conditions: Temperature = 448 °C Volume of the container = 2.0 L 0 = 1 mole H2 (g) = 1 mole I2 (g) 00 00 .. 00 00 •. What is the initial molar concentration of hydrogen. [H:]? What is the initial molar concentration of iodide, [I2]? M This system will reach equilibrium when rate of the forward reaction is equal to the rate of the reverse reaction. Write the equilibrium constant expression, Kc, for this reaction: Calculate the equilibrium concentrations for H;(g), I (g) and HI (g) H2(g}_ + l2 (g) 2 HI (g) [H2] [L2] [HI Initial Change Equilibrium +2x -X-
Initial (M) Change (M) Equilibrium (M) Consider the reaction of SO₂ and O₂ described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 SO₂(g) + O₂(g) = 2 SO₂(g) NEXT A 2.00 L reaction vessel was filled 0.0432 mol SO₂ and 0.0296 mol O₂ at 900 K and allowed to react. At equilibrium, the concentration of SO, was found to be 0.0175 M. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. -0.00875 0.0209 0 0.00875 2SO₂(g) Question 20 of 33 2.00 0.0216 0.0432 0.0148 0.0296 0.0041 O₂(g) 0.0175 2 0.0129 -0.0175 0.0061 RESET -0.0350 0.0257 2SO₂(g)
A chemical engineer is studying the following reaction: N2(9)+3H,(g) → 2NH,(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.00029. The engineer charges ("fills") three reaction vessels with nitrogen and hydrogen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction compound pressure expected change in pressure vessel N2 52.94 atm f increase OI decrease (no change) H2 23.44 atm O t increase OI decrease O (no change) A NH3 14.08 atm O t increase I decrease (no change) N2 47.16 atm O f increase I decrease (no change) В H2 20.07 atm O f increase O I decrease (no change) NH3 11.95 atm O f increase OI decrease (no change) N2 47.80 atm O f increase OI decrease (no change) H2 21.97 atm O f increase OI decrease (no…
The equilibrium constant, Kc, for the following reaction is 57.6 at 277 K. 2CH₂Cl₂ (g) CH4 (9) + CCl4 (9) When a sufficiently large sample of CH₂Cl₂ (g) is introduced into an evacuated vessel at 277 K, the equilibrium concentration of CC14 (g) is found to be 0.383 M. Calculate the concentration of CH₂Cl₂ in the equilibrium mixture. [CH₂Cl₂] = M
At a certain temperature, the reaction: PCl5(g) ⇆ PCl3(g) + Cl2(g) has an equilibrium constant Kc = 6.7E-6. Calculate the equilibrium concentration of PCl3 if only PCl5 is present initially at a concentration of 0.30 M. Your answer should have two significant figures.
Bromine monochloride is synthesized using the reaction Br₂ (g) + Cl₂(g) = 2 BrCl(g) Kp = 1.1 x 10-4 at 150 K A 208.0 L flask initially contains 0.953 kg of Br₂ and 1.184 kg of Cl₂. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: What is the percent yield of BrCl? percent yield: 6.D g %
A mixture initially contains A, B, and C in the following concentrations: [A] = 0.400 M , [B] = 1.40 M , and [C] = 0.300 M. The following reaction occurs and equilibrium is established: %3D %3D A + 2B = C At equilibrium, [A] = 0.270 M and [C = 0.430 M. Calculate the value of the equilibrium constant, K. Express your answer numerically. • View Available Hint(s) ΑΣφ Kc =
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Daniela A chemical engineer is studying the following reaction: 2 H,S(g)+302(g) → 2 SO2(g)+2H,O(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 2.0. The engineer charges ("fills") four reaction vessels with hydrogen sulfide and oxygen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel compound expected change in pressure pressure H, S 1.52 atm O t increase O I decrease O (no change) 0, 8.80 atm O t increase O I decrease O (no change) A so, 9.53 atm O t increase O I decrease O (no change) H,0 5.94 atm O f increase O I decrease O (no change) H, S 0.79 atm O t increase O I decrease O (no change) 6.91 atm Ot increase O l'decrease O (no change) so, 8.61 atm O t increase O I decrease O (no change) H,0…
The equilibrium constant Ke for the reaction PCI3 (9) + Cl2 (g) = PCI, (g) equals 3.5 at 310°C. a A sample of 38.1 g of PCl; is placed in a 2.1 L reaction vessel and heated to 310°C. What are the equilibrium concentrations of all of the species? [PCI5] = | M [PCI3] = | |M [CL] = [ M
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