Calculate AH for the reaction: 6 C(s) + 6 H2(g) + 3 O2(g) → C6H12O6(s) using the following three equations: C(s) + O2(g) → CO2(g) H2(g) + O2(g) → H₂O(1) C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(1) AH°=-285.8 kJ AH° = -285.8 kJ AH°=-2803.02 kJ

Acetic acid. CH3CO2H, is made industrially by the reaction of methanol and carbon monoxide. CH3OH () + CO(g) CH3CO2H() rH= 134.6 kJ/mol-rxn What is the enthalpy change for producing 1.00 L of acetic acid (d = 1.044 g/mL) by this reaction?

The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)

Calculate the standard enthalpy of formation of N2O5 (g) from N2 (g) and O2 (g), in kJ. mol-1, from the following data:                                                                   2NO(g) + O2(g) ® 2NO2(g)      DH = -114.1 kJ 4NO2(g) + O2(g) ® 2N2O5(g)   DH = -110.2 kJ N2(g) + O2(g)  ® 2NO(g)           DH = +180.5 kJ

appendix 4 provides the information deltaH H2 =0kJ/mol deltaH CH4 =-75kJ/mol delta HCl =-92kJ/mol

The average bond energy (enthalpy) for a C=C double bond is 614 kJ/molkJ/mol and that of a C−C single bond is 348 kJ/molkJ/mol. If it takes 4.42×10−19 J/molecule to break the C=C double bond. What is the longest wavelength λ of light that will provide photons of sufficient energy to break the π bond and cause the isomerization? Express your answer numerically in nanometers.

What is the Born-Haber process and how is it important to the world’s economy

Power Index = 178% Heat of explosion (Qv) = 6666kJ/kg Gaseous products detected: CO2, H2O, and N2 (no other gases detected) Total moles of gaseous products detected: 5.3 moles You must determine the molar mass of this compound and draw a reasonable Lewis structure for it. (Hypothetical)

Acetylene (C2H2) and nitrogen (N2) both contain a triplebond, but they differ greatly in their chemical properties.(a) Write the Lewis structures for the two substances. (b) By referring to Appendix C, look up the enthalpies of formationof acetylene and nitrogen. Which compound is more stable?(c) Write balanced chemical equations for the completeoxidation of N2 to form N2O5(g) and of acetylene to formCO2(g) and H2O(g). (d) Calculate the enthalpy of oxidationper mole for N2 and for C2H2 (the enthalpy of formationof N2O5(g) is 11.30 kJ/mol). (e) Both N2 and C2H2 possesstriple bonds with quite high bond enthalpies (Table 8.3).Calculate the enthalpy of hydrogenation per mole for bothcompounds: acetylene plus H2 to make methane, CH4;nitrogen plus H2 to make ammonia, NH3.

32   Use the average bond energies to calculate the ∆H of the reaction:  4H--Cl + O2 → 2H—O—H + 2 Cl—Cl  Data:  ∆H (H-Cl) = 431 kj/mol  ∆H (O-H) = 463 kj/mol  ∆H (O2) = 494 kj/mol  ∆H (Cl-Cl) = 243 kj/mol a. -130 b. -120 c. -150 d. -180