can be calculat EX2 :An equal number of moles of A and B is injected in a reactor (0.5 liters, 1000K) and the equilibrium Ag + Bg > Cg + Dgj is established. At equilibrium the total number of moles is 3.0 and the partial pressure of D is 144.8 atm. a) Calculate the moles of A that should be injected (T=constant) in order to achieve an equilibrium concentration of D equal to 2.0 M b) Briefly describe Le Chatelier's principle providing one example.

can be calculat EX2 :An equal number of moles of A and B is injected in a reactor (0.5 liters, 1000K) and the equilibrium Ag + Bg > Cg + Dgj is established. At equilibrium the total number of moles is 3.0 and the partial pressure of D is 144.8 atm. a) Calculate the moles of A that should be injected (T=constant) in order to achieve an equilibrium concentration of D equal to 2.0 M b) Briefly describe Le Chatelier's principle providing one example.

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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Calculate the Keg from the given concentrations, all are gases. C2H6 1.000 M 2 Cl2 1.000 M C2H4CI2 + 0.000 M 0.250 M + 2 HCI start: 0.000 M equilibrium: 0.750 M 0.500 M 0.500 M 0.500 M used First put in the chemicals, then put in the numbers. The concentrations for both Cl2 and HCl are squared due to their coefficients. [ Kea %3D Keg = a. H3O*1 b. Он1 c. C2H6 d. C2HĄCI2 e. Cl2 f. HCI g. H2SO3 h. HC2H3O2 i. C2H3O21 j. H2S k. HS-1 I. s2 m. HX п. X1 o. 0.750 р. 2 q. 1 r. 0.250 s. 0.500 t. 0.333 u. 8.00 х 10-5 v. 1.75 x 10-6 w. 1.11 x 10-8 x. 5.5 x 10-2 у. О.7000 z. 1.60 x 10-5 aа. 1.143 х 10-5 bb. 0.6000 СС. 1.104 х 10-5 dd. 0.7100 ее. 1.26 х 10-5 ff. 4.901 gg. 7.93 hh. 4.942 ii. 4.957
Consider the reaction of N₂O 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. NEXT > A 1.00 L reaction vessel was filled with 0.0560 mol O₂ and 0.200 mol N₂O and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO2 present. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. Initial (M) Change (M) Equilibrium (M) 0.0100 0.0410 0 -0.0100 0.0710 1 2 N₂O(g) + 3 O₂(g) = 4 NO2(g) 2N₂O(g) 0.0560 -0.0050 0.0360 0.200 0.0050 0.180 + -1.00 0.0150 30₂(g) 2 -0.0560 -0.0150 0.0200 0.210 4NO₂(g) RESET -0.0200 0.190 +
COWLv2 | Online teaching and learning resource from Cengage Le... Consider the reaction: K= [Review Topics] [References] Use the References to access important values if needed for this question. P(s) + 3/2Cl₂ (g) → PCl3 (g) In progress Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K2, for the reactions below: P(s) + 5/2Cl₂ (g) PC13 (9) + Cl₂ (g) For answers with both a subscript and a superscript, enter the subscript first. For example, enter K if the first equilibrium constant should be squared. Submit Answer PC15 (9) K₁ 55 PC15 (g) K₂ b Home | bartleby Retry Entire Group 9 more group attempts remaining C +
Based on a Kc value of 0.170 and the data table given, what are the equilibrium conversations of XY, X, and Y, respectively?
Answer the following:
The equilibrium constant, Kc, for the following reaction is 1.25 at 659 K. 2NH3 (9) N2(g) + 3H₂(g) When a sufficiently large sample of NH3(g) is introduced into an evacuated vessel at 659 K, the equilibrium concentration of H₂(g) is found to be 0.609 M. Calculate the concentration of NH3 in the equilibrium mixture. [NH3] = Submit Answer Use the References to access important values if needed for this question. M Submit Answer Retry Entire Group 8 more group attempts remaining [Review Topics] [References] Use the References to access important values if needed for this question A student ran the following reaction in the laboratory at 679 K: H₂(g) + I₂(g) → 2HI(g) When she introduced 0.208 moles of H₂(g) and 0.237 moles of I2 (g) into a 1.00 liter container, she found the equilibrium concentration of I2 (g) to be 0.0625 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = | Retry Entire Group 8 more group attempts remaining'
Dd.69.
As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°C
Show work..don't give Handwritten answer....don't use Ai for answering this
5. Consider the equilibrium where Kc = 85.0 at 460°C. The following mixture was prepared in a reactor at 460 °C with the concentrations [SO2] = 0.0200 M; [NO2] = 0.0200 M; [NO] = 0.100 M; [SO3] = 0.100 M. What will the concentrations of the four gases be when equilibrium is reached? SO2 (g) + NO2 (g) - NO (g) + S03 (g); Ke = 85.0 I 0.02 O. 02 C -x E 6.02- 0,02-0 0.ltx 0.lto 一× +x 十 LNOJ CSOPJ ) T02=x)co-02-) కంటె CN6 kc
Consider the following reaction at equilibrium. 4CuO (s) + CH4 (8) CO₂ (g) + 4Cu (s) + 2H₂O(g) AH = -514 kJ Le Châtelier's principle predicts that the equilibrium partial pressure of H₂O(g) can be decreased by removing Cu adding CH4 decreasing the reaction temperature decreasing the reactor volume adding an inert gas