Consider the following data. MgS(s)  Mg(s) + S(s)   H = +598.0 kJ SO2(g)  S(s) + O2(g)   H = +296.8 kJ 3 Mg(s) + SO2(g)  MgS(s) + 2 MgO(s)   H = -1504.6 kJ Use Hess's law to calculate (delta)H for the reaction below. 2 MgO(s)  2 Mg(s) + O2(g) (delta)H = ______ kJ

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

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)

Find the ΔH (in kilojoules) for the reaction below, given the following reactions and subsequent ΔH values: (Write your answer in 1 decimal place without the unit). N2(g) +  2O2(g)  →  2NO 2(g) N2(g)  +  3H2(g)  →  2NH3(g)                                  ΔH = -115 kJ 2NH3(g)  +  4H2O(l)  →  2NO2(g)  +  7H2(g)          ΔH = -142.5 kJ H2O(l)  →  H2(g)  +  1/2O 2(g)                                 ΔH = -43.7 kJ

When HCI(g) reacts with O₂(g) according to the following reaction, 28.6 kJ of energy are evolved for each mole of HCI(g) that reacts. Complete the following thermochemical equation. 4HCI(g) + O₂(g)2H₂O(g) + 2Cl₂(g) ΔΗ = 28.6| kj

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

Using the provided table, determine the molar enthalpy (in kJ/mol) for the reaction C₃H₈ (g) + 5 O₂ (g) → 3 CO₂ (g) + 4 H₂O (g) Substance     ∆Hf° (kJ/mol) C₃H₈ (g)             -108.4 O₂ (g)                    0 CO₂ (g)              -393.5 H₂O (g)               -241.8

When a 7.41-g sample of solid potassium chlorate dissolves in 59.3 g of water in a coffee-cup calorimeter (see above figure) the temperature falls from 22.00 oC to 12.96 oC. Calculate H in kJ/mol KClO3 for the solution process. KClO3(s)  K+(aq) + ClO3-(aq)   The specific heat of water is 4.18 J/g-K.Hsolution = _________ kJ/mol KClO3.