Dd.59.I need part A and C please...... ▼For the following reaction, K = 255 at 1000 K.CO (g) + Cl₂ (g) = COCl₂ (g)If a reaction mixture initially contains a CO concentration of 0.1550 M and a Cl₂ concentration of 0.171 M at 1000 K. What is the equilibriumconcentration of CO at 1000 K?Express your answer in molarity to three significant figures.View Available Hint(s)[CO] =SubmitPart BΠ| ΑΣΦ 1X Incorrect; Try Again; 4 attempts remainingPrevious Answers Request Answer[Ch₂] =What is the equilibrium concentration of Cl₂ at 1000 K?Express your answer in molarity to three significant figures.View Available Hint(s)[5] ΑΣΦPart C?→ O[COCI₂] =?MMWhat is the equilibrium concentration of COCl₂ at 1000 K?Express your answer in molarity to three significant figures.►View Available Hint(s)FVTI ΑΣΦ?M

Answered: Image /qna-images/answer/53478e54-3bfe-4720-a29e-d3750b8c6ca9.jpg

▼ For the following reaction, K = 255 at 1000 K. CO (g) + Cl₂ (g) = COCl2 (g) If a reaction mixture initially contains a CO concentration of 0.1550 M and a Cl₂ concentration of 0.171 M at 1000 K. What is the equilibrium concentration of CO at 1000 K? Express your answer in molarity to three significant figures. View Available Hint(s) [CO] = Submit Part B —| ΑΣΦ | 1 X Incorrect; Try Again; 4 attempts remaining Previous Answers Request Answer [Ch₂] = What is the equilibrium concentration of Cl₂ at 1000 K? Express your answer in molarity to three significant figures. View Available Hint(s) [ΕΙ ΑΣΦ ? Part C 3 → C GHIC ? M M What is the equilibrium concentration of COCl₂ at 1000 K? Express your answer in molarity to three significant figures. ►View Available Hint(s) τVE| ΑΣΦ ?

▼ For the following reaction, K = 255 at 1000 K. CO (g) + Cl₂ (g) = COCl2 (g) If a reaction mixture initially contains a CO concentration of 0.1550 M and a Cl₂ concentration of 0.171 M at 1000 K. What is the equilibrium concentration of CO at 1000 K? Express your answer in molarity to three significant figures. View Available Hint(s) [CO] = Submit Part B —| ΑΣΦ | 1 X Incorrect; Try Again; 4 attempts remaining Previous Answers Request Answer [Ch₂] = What is the equilibrium concentration of Cl₂ at 1000 K? Express your answer in molarity to three significant figures. View Available Hint(s) [ΕΙ ΑΣΦ ? Part C 3 → C GHIC ? M M What is the equilibrium concentration of COCl₂ at 1000 K? Express your answer in molarity to three significant figures. ►View Available Hint(s) τVE| ΑΣΦ ?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.41PAE: Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go...

See similar textbooks

Similar questions

Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.
What is the approximate value of the equilibrium constant KP for the change C2H5OC2H5(l)C2H5OC2H5(g) at 25 C. {Vapor pressure was described in the previous Chapter on liquids and solids; refer back to this chapter to find the relevant information needed to solve this problem.)
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.
Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?
Consider the following reaction at 250C: A(s)+2B(g)C(s)+2D(g) (a) Write an equilibrium constant expression for the reaction. Call the equilibrium constant K1. (b) Write an equilibrium constant expression for the formation of one mole of B(g) and call the equilibrium constant K2. (c) Relate K1 and K2.
Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of A(NO3)2 is made to react with 25.00 mL of 0.195 M NaOH. A precipitate, A(OH)2, forms. Along with the precipitation, the temperature increases from 24.8C to 28.2C. What is H for the precipitation of A(OH)2? The following assumptions can be made. â€¢ The density of the solution is 1.00 g/mL. â€¢ Volumes are additive. â€¢ The specific heat of the solution is 4.18 J/g C.
For the reaction N2(g)+3H2(g)2NH3(g) show that Kc = Kp(RT)2 Do not use the formula Kp = Kc(RT)5n given in the text. Start from the fact that Pi = [i]RT, where Pi is the partial pressure of substance i and [i] is its molar concentration. Substitute into Kc.
The equilibrium constant for the butane iso-butane equilibrium at 25 C is 2.50. Calculate rG at this temperature in units of kJ/mol.
A common type of reaction we will study is that having a very small K value (K 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be perfomed. However, the math involved when solving equilibrium problems for reactions having small K values (K 1) is simplified. What assumption is made when solving the equilibrium concentrations for reactions with small K values? Whenever assumptions are made, they must be checked for validity. In general, the 5% rule is used to check the validity of assuming x (or 2 x, 3x, and so on) is very small compared to some number. When x (or 2 x. 3x. and so on) is less than 5% of the number the assumption was made against, then the assumption is said to be valid. If the 5% rule fails, what do you do to solve for the equilibrium concentrations?
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?