In the following reaction, how much heat (in kJ) is released when 4.09 moles of CH₄ are burned? CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O(g) ∆H° = -802 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

In the following reaction, how much heat (in kJ) is released when 5.63 moles of CH₄ are burned? CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O(g) ∆H° = -802 kJ/mol

In the following reaction, how much heat is generated when 2.53 moles of CH₄ are burned? CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O(g) ∆H° = -802 kJ/mol