The nitrogen atoms in an N2 molecule are held together by a triple bond; use enthalpies of formation in Appendix C to estimate the enthalpy of this bond, D(N‚N).

1. Write the enthalpy of formation (AH) for C6H₁2O6(s).

22. Given that the enthalpy of neutralization for the reaction of HCl (a strong acid) and NaOH (a strong base) is always -55.90 kJ per mole of H2O formed, what is the concentration of a 65 mL sample of HCl if the enthalpy of neutralization for the reaction was found to be -5.38 kJ, assuming no heat is lost to the calorimeter?       0.96 M     1.48 M     1.60 M     0.38 M     4.63 M

Hydrazine, N3H4, is a colorless liquid used as a rocket fuel. What is the enthalpy change for the process in which hydrazine is formed from its elements? N3(9) + 2H2 (9) + N2H4 (1) Use the following reactions and enthalpy changes: N2H, (1) + O2 (9) + N2(9) + 2H, 0(1); AH = -622.2 kJ H2 (9) +O2(g) H20(1); AH = -285.8 kJ ΔΗ- k)

7. Calculate the enthalpy of the following reaction. FL + HBr + H₂O 5 so OH Br + HI + HF

When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of iron(II) chloride (FeCl2, molar mass = 126.75 g/mol) and 6.8 kJ of heat is produced. What is the enthalpy change for the reaction when 1 mole of iron(II) chloride is produced? round to sig figs

Use the indicated average bond enthalpies to estimate the change in enthalpy, ΔHo, for the reaction between methane and iodine to produce iodomethane and hydrogen iodide: CH4(g)  +  I2(g)  →  CH3I(g)  +  HI(g)       ΔHo = ? It may be helpful to draw the Lewis electron dot structure for each reactant and product; all reactants and products have single bonds. average bond enthalpies (kJ) C - H  413   ,   C - I  240   ,   H - I  299   ,   I - I  151 Express your answer in units of kilojoules, but do not include the units on your submitted answer.

The Sun supplies about 1.0 kilowatt of energy for each squaremeter of surface area (1.0 kW/m2, where a watt = 1 J/s).Plants produce the equivalent of about 0.20 g of sucrose(C12H22O11) per hour per square meter. Assuming that thesucrose is produced as follows, calculate the percentage ofsunlight used to produce sucrose.12 CO2(g)+ 11 H2O(l)-----> C12H22O11 + 12 O2(g)ΔH = 5645 kJ

(a) Draw a Lewis diagram for carbonic acid, H,CO3, with a central carbon atóm bonded to the three oxygen atoms. (b) Carbonic acid is unstable in aqueous solution and converts to dissolved carbon dioxide. Use bond enthal- pies to estimate the enthalpy change for the following reaction: H,CO;→ H,O + CO,

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