2C6H6() + 15 O2(g) – 12 CO2(g) + 6 H20(/) AH = -5.884 x 103 kJ - An unknown amount of C6H6(/) was combusted in a particular experiment, and the heat released from that reaction was measured to be -6.34 x 103 kJ at constant pressure. Determine the mass (in g) of O2(g) that was consumed during this experiment.

In a popular television series, the two characters use thermite to assist with breaking into a chemical storage facility because the reaction between aluminum and iron(III) oxide produces a tremendous amount of heat. If they began with 10.0 g of Al, how many kJ of heat would be released? 29. 2 Al(s) + Fe,O3(s) → Al,O;(s) + 2 Fe(s) AH = -852 kJ 158 kJ A) B) 236 kJ 472 kJ D) None of the above

When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)

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

At constant volume, the heat of combustion of a particular compound is −3733.0 kJ/mol.−3733.0 kJ/mol. When 1.361 g1.361 g of this compound (molar mass=185.51 g/mol)(molar mass=185.51 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter, including its contents, rose by 8.567 ∘C.8.567 ∘C. What is the heat capacity (calorimeter constant) of the calorimeter?

Consider the following reaction: 2Mg(s)+O2(g)⟶2MgO(s)ΔH∘=−1203kJ What mass of magnesium must be combusted in order to generate 174.0 kJ of heat?

Consider the following equation for the combustion of H₂: 1 H₂(g) + H₂(g) + O₂(g) → O₂(g) → H H₂O(g) + 243 kJ In order to produce 972 kJ of heat, what mass of H₂ must burn?

The flame in a torch used to cut metal is produced by burning acetylene (C2H2)(26.04 g/mol) in pure oxygen. Assuming the combustion of 1 mole of acetylene releases 1251 kJ of heat, what mass of acetylene is needed to cut through a piece of steel if the process requires 22.5  × 104 kJ of heat?                                            2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(g) ΔH = –2502 kJ

In a coffee cup calorimeter with a heat capacity of 21.5 J/ºC, 225 mL of 0.20 M KOH at 22.3 ºC neutralizes 225 mL of 0.20 M HCl at 22.3 ºC. After the reaction occurs, the temperature of the resulting mixture is 29.2 ºC. The density of the final solution is 1.00 g/mL and the specific heat is 4.18 J/g°C. Calculate the Heat of neutralization of KOH.

8. Instant cold packs can be made from ammonium nitrate by mixing/reacting it with water (reaction shown below). When 1.25 g of NH4NO3 is dissolved in 25.0 g of water at 25.8 °C, the temperature of the water after the reaction is 21.9 °C. What is the enthalpy change (ΔH) for this reaction in units of kJ/mol of NH4NO3? The heat capacity of water is 4.18 ?/ ?℃ . NH4NO3(s)  → NH4+(aq) + ??3 − (aq)