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- +) b) H30 H2OS CO₂H Br₂ ACOH▼ Part B 2NO3(aq) +8H(aq) + 6e 3Fe(s) + 2NO3 (aq) +8H+ (aq) 3Fe(s)→→3Fe²+ (aq) + 6e →>> 2NO(g) + 4H₂0 (1) →3Fe²+ (aq) + 2NO(g) + 4H₂O(1) IVE ΑΣΦ Calculate El using the tabulated standard electrode potentials at 25 °C. cell Express your answer in volts to three significant figures. Eeell= 1.21 SWE Submit Previous Answers Request Answer 2+ X Incorrect; Try Again; 4 attempts remaining ? V stontiol buoubtrooting the electro na
- CH,(9) + 2 0,(g) AH = -809.0 kJ/mol rxn co,(9) + 2 H,O(9) ΔΗ. = -81.3 kJ 'cond 2 H,0() Given the energy diagram above (F16-1-3 in the eBook), is the combustion of methane exothermic or endothermic? endothermic exothermic O it could be eitherGiven the following data: 2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(l) ΔG0= -6399 kJ C(s) + O2(g) → CO2(g) ΔG0= -394 kJ H2(g) + ½O2(g) → H2O(l) ΔG0= -237 kJ Calculate the ΔG0rxn for the reaction 6 C(s) + 3 H2(g) → C6H6(l)None
- Predict whether A S for each reaction would be greater than zero, less than zero, or too close to zero to decide.(c) The same weight of methane is more efficient than ethane. True or false? True O FalseGiven the following data: 4C(s) + 4H2(g) + O2(g) → CH3CH2OCOCH3(l) ΔH°=-480.0 kJ CH3CH2OH(l) + O2(g) → CH3COOH(l) + H2O(l) ΔH°=-492.0 kJ 2C(s) + 3H2(g) + 1/2O2(g) → CH3CH2OH(l) ΔH°=-278.0 kJ H2(g) + 1/2O2(g) → H2O(l) ΔH°=-286.0 kJ calculate ΔH° for the reaction:CH3COOH(l) + CH3CH2OH(l) → CH3CH2OCOCH3(l) + H2O(l)
- Using the equations N₂ (g) + 3 H₂ (g) → 2 NH₂ (9) AH° = -91.8 kJ/mol C(s) + 2 H₂(g) →→ CH₂ (g) AH° = -74.9 kJ/mol H₂(g) + 2 C(s) + N₂ (g) → 2 HCN (g) AH° = 270.3 kJ/mol - Determine the enthalpy (in kJ/mol) for the reaction CH₂(g) + NH₂(g) → HCN (g) + 3 H₂ (g).NO2 H NaOH NO2For a particular isomer of Cg H₁g, the combustion reaction produces 5108.7 kJ of heat per mole of Cg H₁ (g) consumed, under standard conditions. C8H18 (g) + -25 0₂(g) →→→ 8 CO₂(g) + 9 H₂O(g) AH; = ΔΗ What is the standard enthalpy of formation of this isomer of Cg H₁8 (g)? 18 -208.5 Incorrect ▲Hixn = -5108.7 kJ/mol kJ/mol
