TUTOR Determining the Equilibrium Constant I Carbon tetrachloride can be produced by the following reaction: CS₂(g) + 3 Cl₂(g) S₂Cl₂(g) + CCl4(9) K= In an experiment, 0.120 mol of CS₂ and 0.360 mol of Cl₂ were placed in a 1.00-L flask at a particular temperature. After equilibrium has been achieved, the mixture contains 0.080 mol CCI4. Calculate the value of K under the experimental conditions. Submit [Reviow Topics Submit Answer Show Approach Show Tutor Steps Retry Entire Group [Refrances) 9 more group attempts remaining

TUTOR Determining the Equilibrium Constant I Carbon tetrachloride can be produced by the following reaction: CS₂(g) + 3 Cl₂(g) S₂Cl₂(g) + CCl4(9) K= In an experiment, 0.120 mol of CS₂ and 0.360 mol of Cl₂ were placed in a 1.00-L flask at a particular temperature. After equilibrium has been achieved, the mixture contains 0.080 mol CCI4. Calculate the value of K under the experimental conditions. Submit [Reviow Topics Submit Answer Show Approach Show Tutor Steps Retry Entire Group [Refrances) 9 more group attempts remaining

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.95QE: Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration...

See similar textbooks

Similar questions

In the text, the equation G=G+RTIn(Q) was derived for gaseous reactions where the quantities in Q were expressed in units of pressure. We also can use units of mol/L for the quantities in Q, specifical.ly for aqueous reactions. With this in mind, consider the reaction HF(aq)H+(aq)+F-(aq) for which Ka = 7.2 104 at 25C. Calculate G for the reaction under the following conditions at 25C. a. [HF] = [H+] = [F] = 1.0 M b. [HF] = 0.98 M, [H+] = [F] = 2.7 102M c. [HF] = [H+] = [F] = 1.0 105 M d. [HF] = [F] = 0.27 M, [H+] = 7.2 104M e. [HF] = 0.52 M, [F] = 0.67 M, [H+] = 1.0 103M Based on the calculated G values, in what direction will the reaction shift to reach equilibrium for each of the five sets of conditions?
The ore cinnabar (HgS) is an important source of mercury. Cinnabar is a red solid whose solubility in water is 5.5 X 10-2 mol L-1. Calculate its \p. What is its solubility' in grams per 100 g of water?
Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.
Withdr... Forms | Office of t... KB Viewing Your Aca.... Have Changes in... Scholarship Ameri... bio 1108 chat [Review Topics] [References] Use the References to access important values if needed for this question. M B # 3 Consider the reaction: P(s) + 3/2Cl₂ (g)=PC13 (g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: 20 E D F3 P(s) +5/2C1₂ (9) PC15 (9) K₁ PCls (g) + Cl₂ (g) =PC15 (9) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter K2 If the first equilibrium constant should be squared. K = C Submit Answer $ 4 988 R F Show Hint % 5 Retry Entire Group 9 more group attempts remaining V Cengage Learning Cengage Technical Support FS T G A 6 MacBook Air B Y H & 7 U N * 0 * 8 J ► 11 FB ( M 9 T 1 K f O O H F10 L A P A command SAVAGE X FENT Next> Save and Exit F12 #1 A ? alt option dele
aland Veterinary. Free income tax Bailey Family Foun.. I Review | Constants | Periodic Table MISSED THIS? Read Section 16.8 (Pages 701 - 710) ; Watch KCV 16.8, IWE 16.9 Equilibrium |0.125 – 1 |0.125 So Consider the reaction [CO2][H3] [CO][H2O] K. = 102 (0.125-z)? CO (g) + H2O (g) = CO2 (g) + H2 (g) K. = 102 at 500 K Since there was no product at the start of the reaction, the final concentration of CO2 is equal to 0 + x = x. A reaction mixture initially contains 0.125 M CO and 0.125 M H2O. Part D What will be the equilibrium concentration of H2? Express the concentration in molarity to three significant figures. ? να ΑΣφ M (H2] =
om/ilrn/takeAssignment/takeCovalentActivity.do?locator%=assignment-take [Review Topics] [References) Use the References to access important values if needed for this question. The equilibrium constant, K. for the following reaction is 1.80×10 at 298 K. NH,HS(s) NH3(g)+ H,S(g) Calculate the equilibrium concentration of H,S when 0.362 moles of NH HS(s) are introduced into a 1.00 L vessel at 298 K. [H,S] =| M Submit Answer Retry Entire Group 8 more group attempts remaining Previous Next 9:14 PM 10/14/202 prt sc delete home end num 8. backspace lock 近
n/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-take E OWlv2 | Online teaching x [Review Topics] [References] Use the References to access important values if needed for this question. The equilibrium constant, K., for the following reaction is 1.80×10 at 298 K. NH,HS(s) NH3(g) + H,S(g) If an equilibrium mixture of the three compounds in a 4.38 L container at 298 K contains 2.09 mol of NHHS(s) and 0.241 mol of NH3, the number of moles of H,S present is moles. Submit Answer Retry Entire Group 8 more group attempts Next 9:14 10/14 近

Brn/takeAssignment/take CovalentActivity.do?locator=assignment-take $ Write the equilibrium constant expression, K, for the following reaction: (If either the numerator or denominator is blank, please enter 1.) 2NOBr(g) 2NO(g) + Br₂ (g) K = Submit Answ F4 % F5 [Review Topics] [References] Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining Cengage Learning Cengage Technical Support A MacBook Air F6 & F7 * DII F8 DD F9 13 F10 Previous * ☐ Next> Save an F
-cnow-owl.cengagenow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator-assignment-take S ot ts This question has multiple parts. Work all the parts to get the most points. [References] Phosphorus pentachloride decomposes at high temperatures. PCl5 (g) PC13 (g) + Cl2 (g) An equilibrium mixture at some temperature consists of 3.56 g of PCl5, 4.86 g of PCl3, and 3.59 g of Cl2 in a 1.00-L flask. a If you add 1.31 g of Cl2, how will the equilibrium be affected? shift left shift right no shift will occur pt pts 1 pt b What will the concentration of PC15 be when equilibrium is reestablished after addition of 1.31 g Cl₂? 1 pt [PC15] = mol/L 1 pt Submit 1 pt 1 pt Submit Answer Try Another Version 4 item attempts remaining ent 80 a F4 F2 F3 # SA % Cengage Learning | Cengage Technical Support F5 1 MacBook Air F6 A DII F7 F8 * A F9
ing and lea X * OWLV2 | Assignment | Finished * OWLV2 | Online teaching and lea X w.com/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-take [Review Topics] [References) Use the References to access important values if needed for this question. Consider the reaction: N2(g) + 2 O2(g)=N204(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K, and K, for reactions a and b below: a.) N204(g) = 2NO2(g) K, b.) 1/2 N2(g) + O2(g)=NO2(g) K = Submit Answer Retry Entire Group 8 more group attempts remaining fho insort sc delete home & 7 8 9 num backspace lock
K GW 16 1. K. for the given reaction at 560 K is 0.0312: a. 2 IBr(g) = 1(g) + Br,(g) Suppose that 1.080 mol IBr is placed in a 1.80 L flask and allowed to reach equilibrium. Determine the equilibrium concentrations of (a) I2; (b) Br;; (c) IBr. (d) What is K,? b. d.
Write the equilibrium expression for the following equation. (Hint: Balance first!) CaCl,(aq) > Ca3(PO4)2(s) + KC(aq) K3PO4(aq) + [Ca3(PO4)2][KCl] Keg= [K3P04][CaCl2] O A. В. [Ca3(PO4)2][KCl]6 Keq= [K3PO4]²[CaCl2]3 O C. Keq= [KCI] [K3PO4][CaCl2] OD. Keq= [KCI]° K PO.12[CaCl]³ hp 96