Please correct answer and don't use hand rating Decide whether each of the molecules in the table below is stable, in the exact form in which it is drawn, at pH = 11.If you decide at least one molecule is not stable, then redraw one of the unstable molecules in its stable form below the table. (If more than one molecule isunstable, you can pick any of them to redraw.)HO40OHOstableO unstable.OHHOstableO unstableXOstableOunstableHOOHOstableO unstable

To determine the stability of each molecule at pH = 11, we need to consider if each functional…

Answered: Decide whether each of the molecules in…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 68QRT

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Similar questions

Write Lewis structures for CO32, HCO3, and H2CO3. When acid is added to an aqueous solution containing carbonate or bicarbonate ions, carbon dioxide gas is formed. We generally say that carbonic acid (H2C03) is unstable. Use bond energies to estimate E for the reaction (in the gas phase) H2CO3CO2+H2O Specify a possible cause for the instability of carbonic acid.
Compound ∆Hf (kJ/mole) ∆S (J/mole K) C2H4 52.4 219.3 C2H6 –84.68 229.2 SiO2 –910.7 41.5 HF –273.3 173.8 SiF4 –1615.0 282.8 NH3 –45.9 192.9 O2 1.88 2.43 NO 91.3 210.8 H2O(g) –241.8 188.8 For the following reactions, using the provided ∆H and ∆S data, determine whether each one would be spontaneous or nonspontaneous at 25°C. C2H4(g) + H2(g) --------à C2H6(g) SiO2 + 4 HF(g) -------------> SiF4 (g) + 2 H2O(g) 4 NH3(g) + 5 O (g) ---------> 4 NO(g) + 6 H2O(g)
Compound ∆Hf (kJ/mole) ∆S (J/mole K) C2H4 52.4 219.3 C2H6 –84.68 229.2 SiO2 –910.7 41.5 HF –273.3 173.8 SiF4 –1615.0 282.8 NH3 –45.9 192.9 O2 1.88 2.43 NO 91.3 210.8 H2O(g) –241.8 188.8 4 NH3 + 5 O2 -> 4 NO + 6 H2O
d) 2SO +Oxe 2S03E) + so (ag) and PbSO Pb The equations above are examples of Homogenous and heterogeneous equilibrium systems Differentiate between Homogenous and Heterogeneous equilibrium. ii) Give the shape and bond angle of the following two molecules BH,NH, and H,0"
← → C Ma esc 2 < Nit Ho Ph Ph 1 app.101edu.co Week 4 Lab-3....docx :0 F1 ^ 2 Ho F2 Use the following table of bond energies to calculate the molar enthalpy of combustion (in kJ/mol) of acetylene (C₂H₂) gas in oxygen, based on the following chemical equation: C₂H₂(g) + 2.50₂(g) → 2CO₂(g) + H₂O(g) 3 HC NO X Single H Bond Gwh Gwh G tar Multiple Bonds 00 80 F3 432 **All values in kJ/mol** 411 346 386 305 167 459 358 W Hy wh (3.ll MA $ 4 000 000 F4 CN O C=C 602 C=O 799 835 C=O 1072 C=C C=N 615 O=O 494 C=N 887 N=N 942 Question 24 of 28 % 5 201 • 142 F5 MacBook Air 6 F6 7 CH AA F7 AP G wh * 8 DII F8 wh 9
Using the table of average bond energies below, the AH for the reaction is kJ. ethanol → ethene + water нн нн Н—С—с—0—н → Ć=Ċ + H-0-H Bond сСС-СО-НС-Н СО AH (kJ/mol) 611 348 464 413 360 -6168 6168 -306 63 46 217
18. (a) Molecule N₂H4 (1) + 2 H₂O2 (1) → N2(g) + 4 H₂O (1) Complete the following table: Lewis Dot Structure (use dots or lines to show bonds) (b) (c) (d) N₂H4 H₂O2 N₂ H₂O Calculate the AH°rxn using average bond energies (Table 9.4 in textbook) Calculate the AH°rxn using the standard enthalpies of formation (Appendix 2 in textbook) Why are these two values slightly different?
How do I do this?
ОН ОН -OH ОН ??? ??? ??? ??? ОН ОН Br ОН
Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on. substance A B C D H chemical symbol, chemical formula or Lewis structure H :0: 44 - C- C-H H - H 1 C I Ar H H | | - C - | 1 H H H Ag H CIO : 0: H boiling point ✓ (Choose one) 1 (highest) 2 3 4 (lowest) (Choose one) ✓ (Choose one) ✓
H2AO4 is a weak acid. What is [AO42 in a 0.30 M H2AO4 solution? [Ka1 = 6.2 x 10-; Ka2 = 5.2 x 10-10 OA21 x 10-5 M OB 5.2 x 10-7 M OC0.60 M OD 6.2 x 10-7 M OE 0.30 M OF 6.2 x 10-10 M OG5.2 x 10-10 M
Bonds Bond Energy (kJ/mol) C-H 411 C-Br 285 H-Br 362 Br-Br 190 Determine ΔH for the reaction: CH4 + 2Br2 ----> CH2Br2 + 2HBr

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