CaO(s)  2 Ca(s) + O2(g)   H = +1270.2 kJ CO2(g)  C(s) + O2(g)   H = +393.5 kJ CaO(s) + CO2(g)  CaCO3(s)   H = -178.3 kJ

Given the standard enthalpies of formation for the following substances, determine the reaction enthalpy for the following reaction. AGran =? kJ 4A (g) + 2B (3) → 1C (g)+ 7D (g) AGi in kJ/mol Substance A (g) B (g) C(g) D (g) 76.34 + 5.24 - 55.86 - 14.55 O - 452.59 kJ/mol O + 452.59 kJ/mol O + 137.17 kJ/mol O - 141.51 kJ/mol O - 137.17 kJ/mol

5.00 g of potassium hydroxide (molar mass = 56.1 g/mol) dissolves in 100.0 g of water and the temperature of the solution increases by 1.60oC. Calculate  ΔH for the reaction in kJ/mol of KOH .The specific heat capacity of the solution is 4.18 J/goC   ( Hint: the mass of the solution is 105g)      (Hint #2: is this + or -?) Your answer should be in kJ/mol and have 3 sig figs

CH1206(s)→3 CH,(g) + 3 CO,(g) AH=-132. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction AH 2C,H1,0,(s) → 6CH,(g) + 6CO,(g) kJ CH,(g) + Co,(g) I kJ 3CH,(g) + 3C0,(g) – C,H1,0g(s) I kJ

Use Hess's Law to calculate the enthalpy for this reaction: 4SO3(g) → 4S(s) + 602(g) AH° ??? kJ !! rxn Given the following thermochemical equations: SO2(g)→ S(s) + O2{g) AH° = +296.8 kJ 2SO2(g) + O2(g) → 2SO3(g) AH° = -197.8 kJ

Given : CH4 (g)  + 2 O2 (g)  -->  CO2 (g) + 2H2O (g)       Δ H = -882 kJ/mol What is Δ H for the reaction below in kJ/mol.    H2O (g)+   1/2  CO2 (g) -->   O2 (g) +  1/2 CH4 (g)

Find the enthapy change for the reaction below in kJ .                   4NH3(g)  + 5O2(g) --> 4NO(g) + 6H2O(g)     ΔH= ?    Given :  (NH3(g)) = -46.1,         (NO(g)) =  + 90.3 kJ/mol   and        (H2O(g)) = -241.8 kJ/mol.

Given the following two equations: 1 S(s) + 2 F2(g) ➞ 1 SF4(g) , ∆H = -774.9 kJ 2 S(s) + 3 O2(g) ➞ 2 SO3(g) , ∆H = -791.44 kJ Calculate the heat change for the reaction: 2 SF4(g) + 3 O2(g) ➞ 2 SO3(g) + 4 F2(g)

Using the table of standard formation enthalpies that you'll find under the ALEKS Data tab, calculate the reaction enthalpy of this reaction under standard conditions: 2 HNO₂(g) + O₂(g) →2 HNO3(g) Round your answer to the nearest kJ. ៣ kJ x10 X

Calculate ΔH orxnfor the following: CH4(g) + Cl2(g) → CCl4(l) + HCl(g)[unbalanced]ΔH o/f[CH4(g)] = −74.87 kJ/molΔH o/f[CCl4(g)] = −96.0 kJ/molΔH o/f[CCl4(l)] = −139 kJ/molΔH o/f[HCl(g)] = −92.31 kJ/molΔH o/f[HCl(aq)] = −167.46 kJ/molΔH o/f[Cl(g)] = 121.0 kJ/mol