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- Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. relative pH of 0.1 M aqueous solution species H20 4 H,PO4 HNO, (Choose one) NO2 7 OH (Choose one) HF (Choose one) ▼1. Fill in the boxes below with the correct reagent, reactant or product (5 (а) OH (b) 1. (CH),СHMgBr 2. H,0 ÓH (c) 1. L¡AIH, 2. НО (d) CH;OH H,SO4 (e) 1. 2 (CH3),CHMgBr, 2. H,0 ÓH (f) 1. LIAIH, 2. H,0 HO,A chemist fills a reaction vessel with 3.61 atm nitrogen (N,) gas, 8.64 atm oxygen (0,) gas, and 6.55 atm nitrogen monoxide (NO) gas at a temperature of 25.0° C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction: N,(g) + O,(g) = 2NO (g) Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule. do Data HNO3 (1) -174.1 HNO3 (g) -133.9 Oxygen OH (aq) H20 (1) -285.8 H20 (g) -241.8 02 (9) H202 (1) -187.8 H202 (9) -136.3 Phosphorus Explanation Check P4 (s) 2021 McC
- 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 D HI chemical symbol, chemical formula or Lewis structure H HH ||| HHH Ar H I Ag -0. H H :O: H |||| HICIC-CIH H boiling point (Choose one) (Choose one) (Choose one) (Choose one)H,0 H,0i Provide the missing curved arrow notation. ס12 + од H C N O S F P C1 Br
- [References] Calculate AH for the reaction: 2NH3 (g) + O2(g) → N2H4 (1) + H2O(1) given the following data: 2NH3 (g) + 3N2O(g) → 4N2(g) + 3H2O(1) AH =–1010. kJ N2O(9) + ЗH2(9) — N;Ha (1) + Hа0(1) ДН %3D — 317 kJ N2H4 (1) + O2 (9) → N2(g)+2H20(1) ΔΗ--623 k.J На (9) + О2(9) — Н,0(1) AH = -286 kJ ΔΗ- kJ Submit Answer Try Another Version 3 item attempts remaining1:25 ul 4G ( Gym buddies HL_DP2.pdf Page 1 of 14 Section A 1. Which equation represents the bond enthalpy for the H-Br bond in hydrogen bromide? A. HBr(g)-H(g)+Br(g) B. HBr(g)-H(g)+Br(1) C. HBr(g)-H(g)+12B12(1) D. HBr(g)-H(g)+12B12(g) 2. Which process is endothermic? A. CH4(g)+202(g)-CO2(g)+2H2O(g) B. HCI(aq)+NaOH(aq)¬NaCI(aq)+H2O(I) C. CaCO3(s)-CaO(s)+CO2(g) D. H2O(g)-H20(1) 3. Hydrazine reacts with oxygen. N2Ha(l) + O2(g) → Na(g) + 2H2O(0) AH = -623 kJ What is the standard enthalpy of formation of NaH«(i) in kJ? The standard enthalpy of formation of H2O(1) is -286 kJ. A. -623 - 286 B. -623 + 572 C.-572 + 623 D. -286 + 623 4. Which statement is correct for this reaction? FezO3 (s) + 3CO (g) - 2Fe (s) + 3CO2 (g) AH = -26.6 kJ A. 13.3 kJ are released for every mole of Fe produced. B. 26.6 kJ are absorbed for every mole of Fe produced. C. 53.2 kJ are released for every mole of Fe produced. D. 26.6 kJ are released for every mole of Fe produced. 5. Which statements are correct? 1. The…NHCOCH3 A NH₂ B Order of electron donating ability (I being the strongest)
