What quantity of heat (in kJ) will be released if 0.3387 mol of NH3 are mixed with 0.200 mol of O₂ in the following chemical reaction? 4 NH3(g) + O₂ (g) → 2 N₂H4 (g) + 2 H₂O (g) AH° = -286 kJ/mol

The standard state of carbon is graphite. ΔH°f,diamond is +1.896 kJ/mol. Diamonds are normally weighed in units of carats, where 1 carat = 0.200 g Determine the standard enthalpy of the reaction for the conversion of a 3.61 -carat diamond into an equivalent mass of graphite.

48.2 mL of a solution of HCl is combined with 110.7 mL of 1.35 M NaOH in a calorimeter. The reaction mixture is initially at 22.4°C, and the final temperature after reaction is 29.3°C. What is the molarity of the HCl solution? You may assume that there is an excess of base (so that all the HCI has reacted), that the specific heat of the reaction mixture is 0.96 cal/g °C, and that the density of the reaction mixture is 1.02 g/mL. The heat of neutralization of HCl and NaOH is 13.6 kcal/mole.

The reaction between HCl and NaOH is represented below. When equal volumes of 1.00 M NaOH and 1.00 M HCl are mixed, 57.1 kJ of heat is released. What would A H be if 2.00 M HCI and 2.00 M NaOH is used instead of 1.00 M? HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l) AH = -57.1 kJ/mol... (A) - 28.6 kJ B-85.7 kJ (c) -57.1 kJ D - 114 kJ

In a constant-pressure calorimeter, 55.0 mL of 0.350 M Ba(OH), was added to 55.0 mL of 0.700 M HCI. The reaction caused the temperature of the solution to rise from 23.81 °C to 28.58 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g °C.) respectively), what is AH for this reaction (per mole H₂O produced)? Assume that the total volume is the sum of the individual volumes. AH= kJ/mol H₂O

In the following reaction, how much heat is generated when 3.21 moles of CH4 are burned? CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O(g) AH° = -802 kJ/mol

How much heat is produced when 57.4 g of NO2 react?    4NO2(g) + O2(g) →  2N2O5(g)      heat of reaction = –110.2 kJ

Determine the amount of heat released when 180.00 g AsBr5(g) reacts according to the following equation: As4O10(g) + 6 AsBr5(g)  →  10 Br3AsO(g) Additional equations that may be useful: 1/4 As4(s) + 3/2 Br2(g)  →  AsBr3(g)  ΔH = -336.4 kJ/mol As4(s) + 5 O2(g)  →  As4O10(g) ΔH = -2967.3 kJ/mol AsBr3(g) + Br2(g)  →  AsBr5(g)  ΔH = -84.2 kJ/mol AsBr3(g) + 1/2 O2(g)  →  Br3AsO(g)  ΔH = -295.7 kJ/mol

25.00 mL of 0.200 M sulfuric acid was added to 25.00 mL of 0.200 M NAOH, in a constant volume calorimeter. The density of the resulting solution is 1.225 g/mL and its specific heat is 5.321 J/g-°C. As the reaction took place, the temperature of the solution rose from 22.0 °C to 31.3 °C. What is AH (in units of kJ/mol) for the reaction, per mole of water formed? This is a limiting reactant problem and your choice of limiting reactant must be justified through stoichiometric calculations. 21.

How much heat is produced when 33.9 g of NO2 react?    4NO2(g) + O2(g) →  2N2O5(g)      heat of reaction = –110.2 kJ