For the reaction A2 + B2 → 2AB, Ea(fwd) = 105 kJ/mol and Ea(rev) = 77 kJ/mol. Assuming the reaction occurs in one step, calculate ΔH°rxn

Consider the following formation reaction.   Ni + 4C + 2O2 → Ni(CO)4 ΔH = -607kJ   What mass of carbon reacts if 45.5 kJ of energy is released?

Does a negative  ΔHᵣₓₙ mean that the heat of reaction can be thought of as a reactant or as a product?

Consider the reaction.   2Fe2O3⟶4Fe+3O2        Δ?∘rxn=+824.2 kJ   The decomposition of 74.0 g of Fe2O3 results in A.) the release of 382 kJ of heat. B.) the absorption of 191 kJ of heat. C.) the release of 191 kJ of heat. D.) the absorption of 30500 kJ of heat. E.) the release of 30500 kJ of heat. F.) the absorption of 382 kJ of heat.

In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.0 rnL of 1.00 M HCI are mixed. Both solutions were originally at 24.6 °C. After the reaction, the final temperature is 31.3 °C. Given that the density of NaCl solution is 1.038 g/mL and the specific heat of NaCl solution is 3.87 J/g-°C, calculate the ΔHneut/mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings.

How much heat (in kJ) will be released (∆H) if 1.20 mol of SrO is mixed with 0.779 mol of CO₂ in the following chemical reaction? SrO (s) + CO₂ (g) → SrCO₃ (s) ∆H° = -234 kJ/mol

2. The decomposition of ammonia gas into nitrogen gas and hydrogen gas is endothermic:   2 NH3 (g) → N2 (g) + 3 H2 (g)     ΔH = 92 kJ/mol   If 762 mL of hydrogen gas, measured at 325°C and 792 mmHg, is formed in the reaction above, how much heat will be absorbed?

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A sample of NaOH (MM = 40.00 g/mol) with a mass of 1.811 g was added to a solution of HNO3 in a coffee cup calorimeter for a final volume of 100.0 mL. If both solutions were initially at 24.5 °C and the temperature of the resulting solution was recorded as 27.0 °C, determine the AH°rxn (in units of kJ/mol NaOH) for the neutralization reaction between aqueous NaOH. Assume that the density and the heat capacity of the resulting solution are the same as water, 1.00 g/mL and 4.184 J/(g x °C) respectively. Your Answer: Answer units

Calculate the change in internal energy (ΔE) for a system that is giving off 3.0 kcal of heat and is changing from 1.00 L to 8.00 L in volume at a pressure of 2.00 atm. (Remember that 101.3 J = 1 L∙atm; 1 cal = 4.18 J)