Determine Kandk,at 298 K for the reaction:NOBR(g) = % N2(g) + O2(g) + % Br2(g)from the following information at 298 K:NO(9) = % N2(g) + % O2(a)Ke = 1.55 x 1015% NO(g) + % Br2(g) = % NOBr(a)Kp = 2.63Type your answers below.Note: If answering in scientific notation, type your answer this way:1.23 x 1045 → type 1.23e45ANSWERS:Kc =Kp =

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Determine KçandKpat 298 K for the reaction: NOBR(g) = % N2{g) + % O2(g) + % Br2(g) from the following information at 298 K: NO(g) ) = % N2(g) + % O2ig) Ke = 1.55 x 1015 ½ NO(g) + % Br2(g) = % NOBr(a) Ko = = 2.63 Type your answers below. Note: If answering in scientific notation, type your answer this way 1.23 x 1045 → type 1.23e45 ANSWERS: Kc = Kp =

Determine KçandKpat 298 K for the reaction: NOBR(g) = % N2{g) + % O2(g) + % Br2(g) from the following information at 298 K: NO(g) ) = % N2(g) + % O2ig) Ke = 1.55 x 1015 ½ NO(g) + % Br2(g) = % NOBr(a) Ko = = 2.63 Type your answers below. Note: If answering in scientific notation, type your answer this way 1.23 x 1045 → type 1.23e45 ANSWERS: Kc = Kp =

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 element chlorine is a useful reagent. For example, it is used for the production of phosgene (carbonyl chloride) from gaseous carbon monoxide CO(g) + Cl2(g) → COCl2(g) Substance COCl2(g) CO(g) Cl2(g) AH (hJL) kJ mol AS (mol·K J - 219.1 283.5 - 110.5 000.0 197.7 223.1 This reaction will be spontaneous at temperatures lower than:
6. Hydrogen sulfide is a pollutant found in natural gas. Following its removal, it is converted to sulfur by the reaction: 2H2S(g) + SO2(9) =Ss(s, rhombic) + 2H20(1) What is the equilibrium constant for this reaction? Is the reaction endothermic or exothermic?
In a constant‑pressure calorimeter, 55.0 mL55.0 mL of 0.900 M H2SO40.900 M H2SO4 was added to 55.0 mL55.0 mL of 0.250 M NaOH.0.250 M NaOH. The reaction caused the temperature of the solution to rise from 22.90 ∘C22.90 ∘C to 24.60 ∘C.24.60 ∘C. If the solution has the same density and specific heat as water (1.00 g/mL1.00 g/mL and 4.184 J/(g⋅°C),4.184 J/(g⋅°C), respectively), what is Δ?ΔH for this reaction (per mole of H2OH2O produced)? Assume that the total volume is the sum of the individual volumes.
While ethanol (CH3CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 25 L tank with 12. mol of ethylene gas and 2.7 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 10.3 mol of ethylene gas and 1.0 mol of water vapor. The engineer then adds another 0.68 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. mol to will Q W x 551 SSA E $ R WS IW an T 6 © 2022 McGraw HILLC. All Rights Reserved. Terms of Use | Privacy Center Accessity Chapter 13- Che...doc CH151 152 Jab .docx Y & 7 H U 8 J ( 9 1 K 1 0 0 A L P + { A 8 @ db Show Al [ 11 1 1 delete
12. For the following reaction at equilibrium in a closed container, ΔΗ-128 kJ 2 NaHCO3 (s) = NażCO3 (s) + H2O (g) + CO2 (g) State the effect (increase, decrease, or no change) of decreasing the temperature on the number of moles of sodium carbonate, Na2CO3. Note that Na2CO3 is a solid (this is a heterogeneous equilibrium); its concentration will remain constant, but its amount can change.
Calculate So values for the following reactions by using tabulated So values from Appendix C.(a) CaCO3(s) CaO(s) + CO2(g)So = ____J/K(b) 2 CH3OH(g) + 3 O2(g) (equilibrium arrow) 2 CO2(g) + 4 H2O(g)So = _____J/K(c) Mg(OH)2(s) + 2 HCl(g)(equilibrium arrow) MgCl2(s) + 2 H2O(l)So = ______J/K(d) 2 PCl3(g) + O2(g)(equilibrium arrow) 2 POCl3(g)So = ____J/K
At -13.0 °C the pressure equilibrium constant K, = 5.8 x 10 for a certain reaction. Here are some facts about the reaction: • Some of the reactants are liquids and solids. • If the reaction is run at constant pressure, the volume increases by 14.%. • The constant pressure molar heat capacity C = 2.03 J· mol. K'. - 1 %3D As Yes. 10 Using these facts, can you calculate K, at 0.80 °C? d. No. If you said yes, then enter your answer at right. Round it to 2 significant digits. Yes, and K, will be bigger. If you said no, can you at least decide whether K¸ at Yes, and K. will be 0.80 °C will be bigger or smaller than K̟ at –13.0 °C? smaller. d. No. Continue Submit Assignment 144H TAKING YOU TO A NEW REALITY et unvmedreabiy PREDATOR
1. Calculate the numerical value of Kc at 193°C for this reaction: 3W (s) + 18 HCI (g) = 3WCl6 (g) +9H₂ (g) 2. At 1225°C, Kc= 2.6x10⁹ for the following reaction: 2BrFs (g) Br₂ (g) + 5F₂ (g) At equilibrium, it is determined that the following are present in a 7.25L container: 0.0333 mole BrF5 0.0777 mole Br₂ How many moles of F₂ are in the container at equilibrium?
For a certain reaction, AGxn = +3.5 kJ/mol at 298 K. %3! a. If this reaction is at equilibrium, which would you expect to have higher concentra- tions: reactants or products?
Use thermochemical data given in the table to decide whether the equilibrium constant for each of the following reactions will increase or decrease with temperature. Substance AH; (kJ/mol) CO(g) CO₂ (g) CS₂(g) CH₁ (9) H₂(g) H₂S(g) H₂O(g) N₂ (9) NH3 (9) O₂(g) -111 -394 117 -74.9 0 -20.5 -242 0 -45.9 0 a. CO₂(g) + H₂(g) → CO(g) + H₂O(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase. b. 2CO2 (g) 2CO(g) + O2(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase.
8. Consider the following equilibrium: 2Cu(s) + O2(g) = 2CUO(s) Kc = ? How would you calculate Kc using the following coupled reactions? 4Cu(s) + O2(g)= 2Cu2O(s) K1 2CuO(s) = Cu2O(s)+ ½ O2(g) K2 KI x K2 CKI x (K2)2 *(K2)2/K1 X(KI)/K2
For a particular reaction △H= -32 kJ and △S = -98J/K (A) At what temp will the reaction be at equilibrium ? (B) If the temperature is increased from the equilibrium temperature what will happen?