If there is a reaction: x OH + a Br2 + b 102 → C Br + d 104 + y H2OUnder alkaline conditions, the values of a, b, c, and d are...........

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Answered: If there is a reaction: x OH + a Br2 +…

If there is a reaction: x OH + a Br2 + b I02 → C Br + d IO4 + y H20 Under alkaline conditions, the values of a, b, c, and d are ...... utl

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

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 102AE: Use the equation in Exercise 79 to determine H and S for the autoionization of water:...

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Use the equation in Exercise 79 to determine H and S for the autoionization of water: H2O(l)H+(aq)+OH-(aq) T(C) KW 0 1.141015 25 1.001014 35 2.091014 40. 2.921014 50. 5.471014
Calculate AH for the reaction, N2H4(1) + O2(g) -----> N2(g) + 2H2O(1), from the following data: 2NH3(g) = 3N20(g) -----> 4N2(g) + 3H2O(1) N20(g) = 3H2(g) 2NH3(g0 + 1/2O2(g) -----> N2H4(1) + H2O(1) H2(g) + 1/2O2(g) AH = -1010 KJ -----> N2H4(1) + H2O(1) AH = -317 KJ AH = -143 KJ %3D -----> H2O(1) AH = -286 KJ
3) One of the main buffer systems found in living organisms is the phosphate buffer system, often used in biological research to mimic cellular conditions. The phosphate equilibrium reactions and their corresponding pKa's are as follows: H3PO4 = H* + H2PO, H2PO, = H+ + HPO?- HPO- = H+ + PO;- pKa1 pКаz —D 7.21 = 12.44 = 2.12 pKa3 (a) Given the above chemical reaction, write out the expression for K, of the buffer system which would predominate at neutral pH conditions. Justify your choice. (b) The human body, and many other lifeforms, prefer an internal pH of 7.2 to maintain homeostasis. However, some more acid-tolerant or basic-tolerant organisms can survive (and sometimes thrive) within different ranges of pH. Calculate the mass and moles of the correct acid and corresponding conjugate base solid (assume you have sodium salts of each base: NaH,PO4, Na,HPO4, and Na PO,) which are needed to make 500 mL of a 0.5 M buffer solution (0.5 M total, including the concentration of acid and base…
8:52 1 ll 5G E Question 24 of 25 Submit Construct the expression for Ksp for solid Ba3(PO4)2 in aqueous solution. Ba3(PO4)2(s) = 3 Ba2"(aq) + 2 PO,3-(aq) 1 Based on your knowledge of how the solid will dissociate in aqueous solution, use the tiles to form the expression. Ksp = 5 RESET [Ba3(PO4)2] 2[Ba3(PO4)2] 3[Ba3(POa)2] [Ba;(PO4)2]? [Ba*] 13 [Ba:(PO.)2] 3[Ba*] [Ba*] [Ba?*] 3[Ba?*] [Ba2*]° [PO,2] 2[PO,²] [PO,2-]? [PO,*] 2[PO.3] [PO,*-]? 3[PO,*-] [PO,³-]³
Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. CH:NH2(aq) + HCIO:(aq)- |3- 2- 4- 2+ |3+ 4+ 1 2 3 4 5 6 7 8 O2 O3 D4 Os |1 6. 10 (s) (1) (g) (aq) + H2O H3O+ H CI OH- C Reset x H2O Delete
determine the Kb for CN- at 25°C. the Ka for HCN is 4.9 x 10^-10
b) а) риденз Ph Brz, Н30 Br₂1 - он 1. LDA, -78 °C 2. ·Br 1. LDA, 20°С 2. Br
26. For each reaction, an equilibrium constant at 298 K is given. Calculate AG for each reaction. a) Br() + H,(g) 2 HBr(g) K,- 4.4 x 10" b) H,O(() = H,O(g) K,= 3.17 x 101 c) N;(g) + 3 Hạ(g) 2 NH,(g) K = 3,5 x 10
6. Calculate the AG for the following reaction at 25 C: (a) N2(g) + O2(g) 2NO(g) (b) H2O1) H2O(g) (c) 2C2H2(9) + 502(g) 4CO2(g) + 2H2Ou) |
52. In ionic solids such as NaCl (salt), the potential energy of a pair CH of ions takes the form U of the ions. For NaCl, a and b have the SI values 4.04×10-28 and 5.52X10-98, respectively, and n = separation in NaCI. = blr" – alr, where r is the separation 8.22. Find the equilibrium
Kk.362.
One mole of a weak acid, HA, was dissolved in 1.9 L of solution. After the system had come to equilibrium, the concentration of HA was found to be 0.42 M. Calculate Ka for НА. K, =