The balanced combustion reaction for C6H6C6H6 is 2C6H6(l)+15O2(g)⟶12CO2(g)+6H2O(l)+6542 kJ2C6H6(l)+15O2(g)⟶12CO2(g)+6H2O(l)+6542 kJ   If 6.100 g C6H66.100 g C6H6 is burned and the heat produced from the burning is added to 5691 g5691 g of water at 21 ∘21 ∘C, what is the final temperature of the water?

When methanol, CH, OH, is burned in the presence of oxygen gas, O,, a large amount of heat energy is released, as shown in the combustion reaction. CH, OH(g) + O₂(g) → CO₂(g) + 2H₂O(1) AH = -764 kJ Based on the balanced thermochemical reaction, how much heat is produced when 25.7 g of methanol reacts with 39.9 g of oxygen? heat: Which reactant is limiting? methanol oxygen kJ

Octane, C3H18 , is a constituent of gasoline, and burns in the presence of oxygen to produce water and carbon dioxide: 25 O2(g) 18 H2O(1) 2 C3H18 (1) + C3H18 (1) → 16 CO2(g) + ΔΗΟ kJ/2mol %D rxn When a 1.00-gram sample of octane is burned in a bomb calorimeter the temperature of the water and the calorimeter rises from 25.00°C to 33.20°C. If the heat capacity, Cpomb cal, of the empty bomb calorimeter is 837 J/°C, and the mass of the water is 1.200 kg: a) Calculate the heat, q, transferred, during the combustion, to the calorimeter: [ Select ] kJ (calorimter) + qbomb cal Cbomb cal • AT b) Calculate the heat, q, transferred, during the combustion, to the water: [ Select ] kJ (1.200 kg H20) + 9H2O = • AT • SH2O + MH20 c) Calculate the enthalpy change (AHº rxn = kJ/2mol) for this reaction (2 mol of C3H18 (1): [ Select ] kJ/2 mol C3H18 (1)

Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3 H₂(g) → 2 NH3(g) ΔΗ= - 92. kJ In the second step, ammonia and oxygen react to form nitric acid and water: NH3(g) + 2O₂(g) → HNO3(g) + H₂O(g) ΔΗ= - 330. kJ Calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ. ☐ kJ X 3

When 130. mL of 0.204 M NaCl(aq) and 130. mL of 0.204 M AgNO3(aq), both at 21.1°C, are mixed in a coffee cup calorimeter, the temperature of the mixture increases to 23.6°C as solid AgCl forms. NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) This precipitation reaction produces 2.71x10³ J of heat, assuming no heat is absorbed by the calorimeter, no heat is exchanged between the calorimeter and its surroundings, and that the specific heat and density of the solutions are the same as those for water (4.18 J/g.°C, and 0.997 g/mL, respectively). Using this data, calculate AH in kJ/mol of AgNO3(aq) for the given reaction. 4.0✔✓ kJ/mol

Consider the following reaction: 2Cr2O3(s)    4Cr(s) + 3O2(g)  DH = 2279.4 kJ Calculate the amount of heat transferred when 6.0 g Cr2O3 (s) of is decomposed by this reaction. How many grams of Cr will form when 6104.2 kJ of heat is absorbed?

In the following reaction how many moles of CH3OH are required to produce -1501 kJ of heat?

Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. In the first step, nitrogen and hydrogen react to form ammonia: N2(g) + 3H2(9) - 2 NH3(g) AH=-92. kJ In the second step, ammonia and oxygen react to form nitric acid and water: NH3(9)+202(9) HNO3(g) + H2O(g) AH -330. kJ Calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ. 10k X 5

calculate the standard enthalpy change (in kJ/mol) for each of the following reactions. (a) 2 Na(s) + I2(g) → 2 NaI(s)  _______________kJ/mol (b) Cr2O3(s) + 3 H2(g) → 2 Cr(s) + 3 H2O(l)  ___________kJ/mol (c) 2 KOH(s) + CO2(g) → K2CO3(s) + H2O(g) _________________ kJ/mol (d) Na(s) + O2(g) → NaO2(s)  _____________kJ/mol

Consider the following reaction. CH3OH(g)  CO(g) + 2 H2(g)    H = +90.7 kJ (a) Is the reaction exothermic or endothermic? exothermic endothermic     (b) Calculate the amount of heat transferred when 55.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H =   kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced?  g(d) How many kilojoules of heat are released when 12.0 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H =   kJ(e) Calculate E when 450.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K