Construct the expression Kc for the following reaction. Sn(s) + 4 Cl:(g) = 2 SnCl-(1) 1 Drag the tiles into the numerator or denominator to form the expression. Each reaction participant must be represented by one tile. Do not combine terms. Kc 5 RESET [SNCL] [CL] [Sn] 2[SnCl] 4[Ch] 2[Sn] [SNCIJF [CLJ* [SnjF 2[SnClJ? 4[CL]* 2[Sn]?

Construct the expression Kc for the following reaction. Sn(s) + 4 Cl:(g) = 2 SnCl-(1) 1 Drag the tiles into the numerator or denominator to form the expression. Each reaction participant must be represented by one tile. Do not combine terms. Kc 5 RESET [SNCL] [CL] [Sn] 2[SnCl] 4[Ch] 2[Sn] [SNCIJF [CLJ* [SnjF 2[SnClJ? 4[CL]* 2[Sn]?

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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owing gas-pr reactions. Average Bond Enthalpies (kJ/mol) Single Bonds C-H C-C C-N C-O C-F C-Cl C-Br C-I C-S C1–C1 Br-Br 413 N-H 348 N-N 293 N-O 358 |N-F 485 N-C1 328 N-Br 276 240 H-H 259 H-F H-Cl H-Br H-I 242 193 Multiple Bonds C=C C=C C=N C=N C=O C=O 391 O-H 163 0-0 201 O-F 272 O-Cl 200 O-I 243 S-H 436 S-F 567 S-Cl 431 S-Br 366 S-S 299 614 |N=N 418 839 |N=N 941 615 |N=O 607 891 799 1072 463 146 190 203 234 339 327 253 218 266 0=0 495
5. Draw a qualitative energy diagram for a two-step reaction with Keq >1. Assume that the first step is slower than the second step. Label fully the reactants, products, transition states, intermediate, activation energies and the net change in energy. Answer:
QUESTION 1 Determine the reaction quotient for the reaction shown below. Select the correct answer below: [CO,J[H,O) [CH][0₂] [CO,][H,O] [CH₂][0,1² [CO,]|H,O] (CH_][O,F [CO][H,O] [CH,110,1¹ Qe= = Qe = CH4 +20₂ CO₂ + 2H₂O
Identify the equilibrium expression for the reaction CH,CHO(g)CH₂(g) + CO(g). [CH,][CO] [CH,CHO] a) K= b)x= [CH,]+[CO] [CH,CHO [CH,CHO] [CH,+[CO] Oc) K- [CH,CHO] Q) d) K= ÍCH][CO] e) x= [CH,CHO][CH,][CO)
Activity 1: Complete Me! Direction: Complete the following table. Write your answer on a separate sheet of paper. Equilibrium Reaction Effect Keq expression Stress Equilibrium shift (encircle your answer) Forward applied (encircle your answer) Ha + Cla = | 2HCI Decreasing the pressure (increase, decrease, no change) in the number (HCIJ Keq - Backward No Shift of moles of HCl(g) (increase, decrease, no change) in the volume of Increasing Fe,O +4 Ha + heat 2 Forward Keq = the Backward 3Fe + 4H,O temperature No Shift water vapor collected of (increase, decrease, no change) the number of moles of NO 2NO + Oz 2NO + heat Forward Backward No Shift Addition (NO,P |NO]F|0,]| Keq = helium Forward H,CO» = CO2 + H,O Removal of (increase, decrease, no change) in the amount Keq - (H,CO, CO2 Backward No Shift of H,CO, (increase, decrease, no change) in amount of o, (increase, the volume of decrease, no change) in the Increasing the Forward Backward No Shift Keq= temperature the 4 NH3%g + 502 2 4NO+ 6…
14. Calculate the Kc of the reaction 2NO (g) + Br2 (g) ---> 2NOBr (g) from the following information: 2 NO(g) ---> N2(g) + O2(g) Kc = 1 × 10^30 N2(g) + Br2(g) + O2(g)---> 2 NOBr(g) Kc = 2x10^-27
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Construct the expression for Kc for the following reaction. H₂O(1) ⇒ H+ (aq) + OH- (aq) Drag the tiles into the numerator or denominator to form the expression. [H₂O] 2[H+] [OH-]² K₂ 1 2[H₂0] [H+]² [H₂O]² [OH-] RESET [H+] 2[OH-]
⦁ 4. Make your own energy diagram for an exothermic reaction that does not include a catalyst and one with a catalyst (Be sure each line is a different color or labeled). Label the axis of the diagram. Then, state what a catalyst is and how a catalyst affects the reaction rate.
Find Ksp expression and value with the information given
47. Consider the reaction: MISSED THIS? Read Section 16.7; Watch KCV 16.7, IWE 16.7 NH4HS(s) NH3(g) + H₂S(8) At a certain temperature, Ke = 8.5 x 10-³. A reaction mixture at this temperature containing solid NH,HS has [NH3] = 0.166 M and [H₂S] = 0.166 M. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?
Consider the methanol synthesis reaction represented below. CO (g) + 2 H2 (g) = CH3OH (g) The initial concentrations were: [CO ] = 1.75 M, [H2] = 1.00 M, and [CH3OH] = 0.65 M. %3D %3D If the equilibrium [CO] was found to be 1.60 M, calculate the equilibirium constant (K) for this reaction. Note: Reaction temperature was kept constant throughout the process. 44 2.0 1.0 62