Please solve all questions otherwise I will dislike .Thank s ASAP 6._C₂H4(g) + O2 (g)=CO₂ (g) + H₂O (1)If 10 moles of ethylene reacts with 9 moles O₂ to produce 2 moles of CO₂ in a 2 L vessel, what is the equilibriumconstant? Are products are reactants favored?bre7. Determine the [H.] and pH of a 0.35M HCl solution.8. Determine the [H] and pH of a 2.00 x 10-5 M H₂SO4 solution.(8) 289. Determine the [H+] and pH of a 0.0052M HCOOH (formic acid) solution.Isupe vieubiyibni [s] bns [H) novig [H] olubles es 18.(2) IHS (8) + (8) to ne0. Determine the [H.] and pH of a 1.5 x 10-2 M HCN (hydrocyanic acid). () 2

Given : 1. Moles of ethylene = 10 moles Moles of O2 = 9 moles Moles of CO2 produced = 2 moles…

6. _C₂H4(g) + O2 (g)=CO₂ (g) +____ _H₂O (1) - If 10 moles of ethylene reacts with 9 moles O₂ to produce 2 moles of CO₂ in a 2 L vessel, what is the equilibrium constant? Are products are reactants favored? ber 7. Determine the [H.] and pH of a 0.35M HCl solution. 8. Determine the [H] and pH of a 2.00 x 10-5 M H₂SO4 solution. (5) 8

6. _C₂H4(g) + O2 (g)=CO₂ (g) +____ _H₂O (1) - If 10 moles of ethylene reacts with 9 moles O₂ to produce 2 moles of CO₂ in a 2 L vessel, what is the equilibrium constant? Are products are reactants favored? ber 7. Determine the [H.] and pH of a 0.35M HCl solution. 8. Determine the [H] and pH of a 2.00 x 10-5 M H₂SO4 solution. (5) 8

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 12.65PAE

See similar textbooks

Similar questions

For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
Explain why a sample of pure water at 40 C is neutral even though [H3O+]=1.7107M . Kw is 2.91014 at 40 C.
Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?
You have a solution of the weak acid HA and add some HCl to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
How is acid strength related to the value of Ka? What is the difference between strong acids and weak acids (see Table 13-1)? As the strength of an acid increases, what happens to the strength of the conjugate base? How is base strength related to the value of Kb? As the strength of a base increases, what happens to the strength of the conjugate acid?
9. A base is added to water and a new equilibrium is established. The new equilibrium can be described by * A. pH pOH and Kw = 1 x 1014 С. рH 1 x 10-14
10. The active ingredient in many toilet bowl cleaners is simply hydrochloric acid. Hydrochloric acid is particularly good at removing rust stains and hard water deposits. One particular brand uses hydrochloric acid at a concentration of 5.800 M. A. B. What is the equilibrium concentration of H₂O* of a pH = 5.172 solution? Please provider your answer below. What is the pH of the 5.80 M HCl solution? Please provider your answer below. ☐☐ S + 00 S C. To what volume would 35.00 mL of this brand have to be diluted for the final solution to have a pH = 1.20? mL Please provider your answer below. M $
A solution containing 2.60 x 10-3 moles of NAOH and 3.32 x 10-3 moles of HCl into a container and then water is added until the final volume is 1.00 L. What is the pH of this solution? (Hint: pH + pOH=14; pH= -log1o [H"] and pOH = -log10 [OH"]) OA. 2.84 О в. 10.86 Oc 11.16 O D. 3.14 O E. 2.50