Using the following thermochemical equation, determine the amount of heat produced per kg of CO2 formed during the combustion of benzene (C6H6). 2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g) ΔH°rxn = -6278 kJ

Given the following thermochemical equations:H2 (g) + F2 (g) → 2HF (g) ΔH = -537 kJC (s) + 2F2 (g) → CF4 (g) ΔH = -680 kJ2C (s) + 2H2 (g) → C2H4 (g) ΔH = +52.3 kJCalculate the ΔH for the reaction of ethylene with F2: C2H4 (g) + 6F2 (g) → 2CF4 (g) + 4HF (g) [Calorimetry]

It is recommended that the average daily intake of glucose for humans is not to exceed 32.5 g of glucose (C6H12O6). The balanced chemical equation for the combustion of glucose is shown below. C6H12O6(aq) + 6 O₂(g) → 6 CO₂(g) + 6 H₂O (1) AH rxn= -1273.3 kJ/mol How much heat is released when 55.5 g of oxygen are combusted with glucose as shown in the reaction. above? Use the provided Periodic Table for any calculations involving elements. Report your answer to a single decimal place and report proper units with your answer.

Natural gas burns in air to form carbon dioxide and water, releasing heat. CH4(g) + O2(g) → CO2(g) + H2O(g)                                    ΔHorxn = -802.3 kJ What minimum mass of CH4 is required to heat 23g of water by 32oC? (Assume 100% heating efficiency.) Natural gas burns in air to form carbon dioxide and water, releasing heat. CH4(g) + O2(g) → CO2(g) + H2O(g)                                    ΔHorxn = -802.3 kJ What minimum mass of CH4 is required to heat 23g of water by 32oC? (Assume 100% heating efficiency.) 62 g 22.5 g 7.80 mg 61 mg 118 mg

The table lists the specific heat capacities of select substances. Substance Specific heat capacity (J/g °C) lead 0.128 silver 0.235 соpper 0.385 iron 0.449 aluminum 0.903 water 4.184 An unknown substance has a mass of 10.5 g. The temperature of the substance increases by 13.3 °C when 53.8 J of heat is added to the substance. What is the most likely identity of the substance? iron lead aluminum copper water silver O O C

Consider the thermochemical equation for the combustion of acetone (C3H₂O), the main ingredient in nail polish remover: C3H6O (1) + 4 O₂ (g) → 3 CO₂ (g) + 3 H₂O (g) ΔΗ° rxn = 1790 kJ If a bottle of nail polish remover contains 222 mL of acetone, what is the magnitude (the value) of heat released by the complete combustion of the acetone in the bottle? The density of acetone is 0.788 g/mL. The molar mass of acetone is 58.08 g/mol. The units are kJ. Do not include units in your answer.

What is the enthalpy change when  2.00 mol of oxygen (O2) react? C12H22O11(s)   + 12 O2(g) →    12 CO2(g)  +    11 H2O(l)        ΔH = -5644 kJ

22.214 g of a metal at 99.73°C was added to 14.2 g of water at 19.05°C. The temperature of the mixture rose to 28.78°C. What is the specific heat of the metal?  SH2O = 4.184 J/g°C

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

33 a b C d e Consider the hypothetical thermochemical equation 3A+B→2C for which AH = 61.5 kJ/mol. L L L L L If you have 5.30 moles of A, what quantity of heat, in kJ, would be absorbed? If the reaction absorbs 345 kJ of heat, What quantity in moles of C would be produced? What would AH, in kJ/mol, be for the reaction 2 C → 3 A + B? What would AH, in kJ/mol, be for the reaction 9A + 3 B →6 C? Which one of the following reactions would have an enthalpy change of -2xAH? Here, AH refers to the enthalpy change of the original reaction.