takeAssignment/takeCovalentActivity.do TripAdvisor Facebook (Review Topics] [References) Use the References to access important values if needed for this question. The equilibrium constant, K, for the following reaction is 7.00×10-5 at 673 K. NH,I(s) NH3(g) + HI(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 673 K contains 0.286 mol NH,I, 8.37x10-3 M NH, and 8.37x10-3 M HI. If the concentration of NH3(g) is suddenly increased to 1.55x102 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = M (HI) M Submit Answer Retry Entire Group 1 more group attempt remaining Previous Next Fmail Instructor Save and Exit

takeAssignment/takeCovalentActivity.do TripAdvisor Facebook (Review Topics] [References) Use the References to access important values if needed for this question. The equilibrium constant, K, for the following reaction is 7.00×10-5 at 673 K. NH,I(s) NH3(g) + HI(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 673 K contains 0.286 mol NH,I, 8.37x10-3 M NH, and 8.37x10-3 M HI. If the concentration of NH3(g) is suddenly increased to 1.55x102 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = M (HI) M Submit Answer Retry Entire Group 1 more group attempt remaining Previous Next Fmail Instructor Save and Exit

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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[Review Topics] [References] Use the References to access important values if needed for this question. The equilibrium constant, Kc, for the following reaction is 7.00 × 10-5 at 673 K. NH4I(s) NH3(g) + HI(g) If an equilibrium mixture of the three compounds in a 6.73 L container at 673 K contains 1.48 mol of NH4I(s) and 0.467 mol of NH3, the number of moles of HI present is mol. Submit Answer Q F4 % 5 Show Hint F5 ^ 6 Y Retry Entire Group 8 more group attempts remaining C F6 & 7 F7 * 8 F8 ( 9 F9 O ) O F10 P F11 Previous + F12 Next> delete
cator=assignment-take Use the References to access important values if needed for this question. The equilibrium constant, K, for the following reaction is 1.20x 10-2 at 500 K. PCI5(9) PC|3(g) + Cl₂(9) An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.242 M PCI5, 5.39x10-2 M PCl3 and 5.39x 10-2 M Cl₂. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.68x 10-2 mol of Cl₂(g) is added to the flask? [PCIs] = IM [PC|3] = M [Cl₂] = M Retry Entire Group 1 more group attempt remaining Previous Next> WEB 48 One Touch Web Access Without Booting Up NumLk Prt Sc Submit Answer SONY Other Bookmarks 4:22 AM 4/30/2022 VGN-NW350F Delete Break
The equilibrium constant, Kc , for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g)If an equilibrium mixture of the three compounds in a 5.09 L container at 548 K contains 3.65 mol of NH4Cl(s) and 0.368 mol of NH3, the number of moles of HClpresent is moles.
The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K. 2HI(g)=H₂(g) + 12(g) An equilibrium mixture of the three gases in a 1.00 L flask at 698 K contains 0.324 M HI, 4.35×10-² M H₂ and 4.35×10-² M I₂. What will be the concentrations of the three gases once equilibrium has been reestablished, if 2.90×10-2 mol of H₂(g) is added to the flask? [HI] = [H₂] = [1₂] ΣΣΣ
The equilibrium constant, K, for the following reaction is 5.00x10-2 at 642 K. COCI2(g) : =CO(g) + Cl2(g) An equilibrium mixture of the three gases in a 5.49 L container at 642 K contains 0.288 M COCI2, 0.120 M CO and 0.120 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 11.9 L? [COCI2] = [CO] [Cl2] M ΣΣΣ Il||
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The equilibrium constant, K, for the following reaction is 10.5 at 350 K.2CH2Cl2 (g) CH4 (g) + CCl4 (g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.43×10-2 M CH2Cl2, 0.176 M CH4 and 0.176 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.143 mol of CH4(g) is added to the flask?
At 500 K, hydrogen and iodine can form hydrogen iodide in the gas-phase reaction: 2HI(g) H₂(g) + 12(g) In one experiment, 0.176 g of HI were placed in an evacuated 1.00 L flask at 500 K, and allowed to come to equilibrium, the final pressure was 0.0893 atm. What were the partial pressures of HI, H2, and 12 and what is the equilibrium constant? Phi = i PH2= i P12 = i Kc = i Deal atm atm atm
The equilibrium constant, Kp, for the following reaction is 1.04x10-² at 548 K. NH4CI(S) NH3(g) + HCl(g) If an equilibrium mixture of the three compounds in a 6.78 L container at 548 K contains 2.85 mol of NH4Cl(s) and 0.113 mol of NH3(g), the partial pressure of HCI(g) is atm.
At a certain temperature, the equilibrium constant, ?c, for this reaction is 53.3. H2(g)+I2(g)↽−−⇀2HI(g)?c=53.3 At this temperature, 0.400 mol H2 and 0.400 mol I2 were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium? [HI]= M At a certain temperature, the equilibrium constant for the chemical reaction shown is 1.13×10−3. At equilibrium, the concentration of AB is 2.725 M, the concentration of BC is 2.225 M, and the concentration of AC is 0.220 M. Calculate the concentration of B at equilibrium. AB(aq)+BC(aq)↽−−⇀AC(aq)+2B(aq) [B]= M
Carbon monoxide and water vapor are formed when carbon dioxide and hydrogen react. CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium constant for the reaction is KC = 2.10 at 247 ℃. If 0.657 mol of carbon dioxide is added to 0.512 mol of hydrogen in a 0.84–L reaction vessel and allowed to react at this temperature, what is the equilibrium concentration (in mol/L) of carbon dioxide? Report your answer to THREE significant figures.
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