help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working! Thinking (20T)1. Calculate AH for the reaction 2 Al (s) + 3 Cl₂ (g) --> 2 AICI 3 (s) from the data.(5marks)2 Al (s) + 6 HCI (aq) --> 2 AICI, (aq) + 3H2(g)HCI (g) -> HCI (aq)--H2 (g) + Cl2 (g) --> 2 HCI (g)AICI, (s)--> AICI, (aq)AH = -1049. KJAH = -74.8 kJΔΗ = - 1845. ΚΙAH = -323. KJ

Enthalpy change is an extensive property. When a multiplier is used on an equation, the enthalpy…

Thinking (20T) 1. Calculate AH for the reaction 2 Al (s) + 3 Cl₂ (g) --> 2 AICI 3 (s) from the data.(5 marks) 2 Al (s) + 6 HCI (aq) --> 2 AICI, (aq) + 3H2(g) HCI (g) -> HCI (aq) -- H2 (g) + Cl2 (g) --> 2 HCI (g) AICI, (s)--> AICI, (aq) AH = -1049. KJ AH = -74.8 kJ ΔΗ = - 1845. ΚΙ AH = -323. KJ

Thinking (20T) 1. Calculate AH for the reaction 2 Al (s) + 3 Cl₂ (g) --> 2 AICI 3 (s) from the data.(5 marks) 2 Al (s) + 6 HCI (aq) --> 2 AICI, (aq) + 3H2(g) HCI (g) -> HCI (aq) -- H2 (g) + Cl2 (g) --> 2 HCI (g) AICI, (s)--> AICI, (aq) AH = -1049. KJ AH = -74.8 kJ ΔΗ = - 1845. ΚΙ AH = -323. KJ

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 6ALQ: Sketch a pH curve for the titration of a weak acid (HA) with a strong base (NaOH). List the major...

See similar textbooks

Similar questions

Calculate the pH of a 1.25 L carbonate buffer which was prepared by mixing 0.1170 M of Na2CO3 and 0.400 M NaHCO3. (Ka of HCO3- = 4.70 x 10-11) pH 9.2 pH 10.8 pH 10.2 pH 9.8
Question 8 of 10 Complete the balanced neutralization equation for the reaction below: H2SO«(aq) + Mg(OH)2(aq)→ 0 4- 3- 0² 2- 2+ 3+ 4+ 2 4 6. 7 8 6. 0. 03 04 1 6. 8. (s) | (I) (g) (aq) H. Mg Reset • x H2O Delete Type here to search hulu
5:50 1 Search Question 5 of 20 Submit Determine the mass of solid NaCH;COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH-COОH is 1.8 х 10-5. 1 2 Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH3COOH+ H20(1) =H;O*(aq) +CH3COO-(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.200 5.00 -5.00 1.0 x 10-9 -1.0 × 10-9 1.0 x 10-5 -1.0 x 10-5 1.8 x 10-5 -1.8 x 10-5 х+ 5.00 x - 5.00 x + 1.0 × 10-9 х - 1.0 х 10-9 1.0 x 10-5 x - 1.0 × 10-5 x + 1.8 × 10-5 х - 1.8 х 10-5
1. A 50.0 mL solution of 0.150 M acetic acid (CH3COOH) is titrated with 0.150 M NaOH. What is the pH after 20.0 mL of base has been added? Ka CH3COOH = 1.8 x 10-5 I attached my answer.
I only need answer not explain 10 mint please
5:51 1 .ll LTE Search Question 16 of 20 Submit Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH, with 0.100 M HNO3 after 80.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. 1 2 4 Based on the result of the acid-base reaction, set up the unknown. ICE table in order to determine the H2NNH3*(at H2O(1) =H;O*(aq) H2NNH2(aq + Initial (M) Change (M) Equilibrium (M) RESET 0.100 0.200 0.0333 0.0667 +x -X 0.100 + x 0.100 - x 0.200 + x 0.200 - x 0.0333 + x 0.0333 - x 0.0667 + x 0.0667 - x www
1 attempts left Check my work Enter your answer in the provided box. A buffer solution is prepared in such a way that the concentration of propanoic acid is 1.8 x 10 M and the concentration of sodium propanoate is 1.9 x 10° M. The buffer equilibrium is described by Guic C,H;COOH(aq) + H2O(1) =H,o*(aq) + C,H3CO0aq) propanoic acid propanoate ion with K 1.34 x 10P. If the concentration of the sodium propanoate were doubled while the acid concentration remained the same, calculate the pH of the resulting solution. pH =
Consider a buffer prepared from the weak acid HCO3¯ and its conjugate base CO3?". HCO3 (aq) + H,0(1) = CO3² (aq) + H3O*(aq) a. What happens to the concentrations of HCO,¯ and CO3²- when a small amount of acid is added to the buffer? [HCO,-] (select) | and [Co,²-] select) b. What happens to the concentrations of HCO3 and CO,?- when a small amount of base is added to the buffer? [HCO, ] (select) | and [Co,²-] (select)
What is the pH of the solution when Caitlin has added 30.00 mL of the 0.25 M LIOH to the 25.00 mL of 0.40 M formic acid? K₂ = 1.8 x 10-4 pH = [?] pH of Solution Enter
Q18
A phosphate buffer contains KH2PO4 and K2HPO4. What is the net ionic equation for the buffering reaction that occurs when some HCl is added to the buffer solution? (A) H2PO4–(aq) + Cl–(aq) --> HPO42–(aq) + HCl(aq); (B) H2PO4–(aq) + H3O+(aq) --> H3PO4(aq) + H2O(aq); (C) HPO42–(aq) + Cl–(aq) --> PO43–(aq) + HCl(aq); (D) HPO42–(aq) + H3O+(aq) --> H2PO4–(aq) + H2O(aq);
See image below. Can you please show me how to solve this, especially with the reaction equation and equilibrium equation (to make the reaction table)? Thank you!!!