# hw 10 - dziewa(jcd935 – Homework#11 – Holcombe...

This preview shows pages 1–2. Sign up to view the full content.

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: dziewa (jcd935) – Homework #11 – Holcombe – (52460) 1 This print-out should have 10 questions. Multiple-choice questions may continue on the next column or page – find all choices before answering. 001 10.0 points The equilibrium constant for the reaction 2 Hg( ℓ ) + 2 Cl − (aq) + Ni 2+ (aq) → Ni(s) + Hg 2 Cl 2 (s) is 5.6 × 10 − 20 at 25 ◦ C. Calculate the value of E ◦ for a cell utilizing this reaction. 1. + 1.14 V 2.- 1.14 V 3.- 0.25 V 4.- 0.57 V correct 5. + 0.57 V Explanation: 002 10.0 points The standard voltage of the cell Ag(s) | AgBr(s) | Br − (aq) || Ag + (aq) | Ag(s) is +0.73 V at 25 ◦ C. Calculate the equilibrium constant for the cell reaction. 1. 4 . 6 × 10 − 13 2. 2 . × 10 − 15 3. 2 . 2 × 10 12 correct 4. 5 . 1 × 10 14 5. 3 . 9 × 10 − 29 Explanation: 003 10.0 points Calculate the reduction potential for the Zn 2+ | Zn electrode if the Zn 2+ concentra- tion is 4 × 10 − 3 M. The standard potential for Zn 2+ + 2 e − → Zn is- . 7628 V. 1.- . 833 V correct 2.- . 904 V 3.- 1 . 666 V 4.- 1 . 808 V Explanation: [Zn 2+ ] = 4 × 10 − 3 M E = E- parenleftbigg . 0592 n parenrightbigg log Q =- . 7628 V- parenleftbigg .....
View Full Document

## This note was uploaded on 09/14/2010 for the course C E 301 taught by Professor Staff during the Spring '08 term at University of Texas.

### Page1 / 3

hw 10 - dziewa(jcd935 – Homework#11 – Holcombe...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document
Ask a homework question - tutors are online