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 is unstable, you can pick any of them to redraw.) Ostable HO Ounstable ? Х OH Ostable E Ounstable HO HO Ostable "Ostable Ounstable Ounstable Explanation Check Х C + © 2024 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility o0o 信 Ar

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 is unstable, you can pick any of them to redraw.) Ostable HO Ounstable ? Х OH Ostable E Ounstable HO HO Ostable "Ostable Ounstable Ounstable Explanation Check Х C + © 2024 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility o0o 信 Ar

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

See similar textbooks

Similar questions

You may want to reference (Pages 187 - 190) Section 5.7 while completing this problem. Part C Using values from Appendix C, calculate the value of AH° for each of the following reactions. 2CuO(s) +NO(g)→CU2O(s) +NO2 (g) Express your answer using three significant figures. ? ΔΗ3 kJ Submit Request Answer Part D 4NH3(g) + O2 (g)→2N2H4(g) +2H2O(1) Express your answer using five significant figures. ? AĦgm = kJ
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
Calculate ΔH° for the reaction using the given bond dissociation energies. CH4(g)+2O2(g)⟶CO2(g)+2H2O(g) Bond ΔH° (kJ/mol) O–OO–O 142 H–OH–O 459 C−HC−H 411 C=OC=O 799 O=OO=O 498 C–OC–O 358 What type of reaction is this?
Calculate AH for the reaction using the given bond dissociation energies. CH,(g)+2O,(g) — CO,(g) +2H,O(g) Bond AH (kJ/mol) 0-0 H-O C-H C=O 0=0 C-O AH° = 142 459 411 799 498 358 A kJ/mol This reaction is exothermic. endothermic.
How do I determine and write out products of this reaction? Also is this a decomposition reaction? NaHCO3 (s) →
At room temperature and 1 atm carbon dioxide (CO2) is a
Gg.143.
The neutralization of a strong acid and strong base has an enthalpy change, ∆H°, = -55.9 kJ/mol. The net ionic equation for this reaction is H⁺(aq) + OH⁻(aq) ⇌ H₂O(l) which is the reverse of the autoionization of water, and therefore ∆H° for the autoionization of water = +55.9 kJ/mol. Kw for the autoionization of water is 1.0 × 10⁻¹⁴ at 25°C. Distilled water has a [H⁺] = 1.0 × 10⁻⁷ M and a neutral pH of 7.0. Calculate the neutral pH of distilled water at 95°C.
According to this figure: HO NH2 HN NH2 NH2 NH3 HO HO What is the type of interaction labeled A? Oal lonic bond
A student determines the value of the equilibrium constant to be 7.94×10-37 for the following reaction.H2S(g) + 2H2O(l)3H2(g) + SO2(g)Based on this value of Keq:G° for this reaction is expected to be (greater, less) than zero.Calculate the free energy change for the reaction of 1.85 moles of H2S(g) at standard conditions at 298K. G°rxn = kJ
We can describe the combustion of glucose, and the accompanying energy change, as. C6H1206+602-6 H₂O+6 CO2, AU=-5670 kJ The molar energy change, expressed in terms of oxygen consumed, is O 945 kJ mol-1. O 5670 kJ mol-1. O-945 kJ mol-1. O-5670 kJ mol-1. O 472 kJ mol-1.