Nitromethane (CH3NO2) burns in air to produce significant amounts of heat. 2 CH3NO2(l ) + 32 O2( g)¡2 CO2( g) + 3 H2O(l ) + N2( g) ΔH °rxn = -1418 kJ How much heat is produced by the complete reaction of 10.47 kg of nitromethane?

Determine whether each process is exothermic or endothermic and indicate the sign of ΔH. a. natural gas burning on a stove b. isopropyl alcohol evaporating from skin c. water condensing from steam Indicate the sign of ΔH for the following processes.

Determine whether each process is exothermic or endothermic and indicate the sign of ΔH. a. dry ice evaporating b. a sparkler burning c. the reaction that occurs in a chemical cold pack used to ice athletic injuries

What mass of natural gas (CH4) must burn to emit 352 kJ of heat? CH4( g) + 2 O2( g)¡CO2( g) + 2 H2O( g) ΔH °rxn = -802.3 kJ

Titanium reacts with iodine to form titanium(III) iodide, emitting heat. 2 Ti(s) + 3 I2( g)¡2 TiI3(s) ΔH °rxn = -839 kJ Determine the mass of titanium that react if 2.38 * 103 kJ of heat is emitted by the reaction.

The propane fuel (C₃H₈) used in gas barbeques burns according to the thermochemical equation: C₃H₈(g) + 5 O₂(g) → 3 CO₂(g) + 4 H₂O(g) ΔH°_rxn = –2044 kJ If a pork roast must absorb 1.6×10³ kJ to fully cook, and if only 10% of the heat produced by the barbeque is actually absorbed by the roast, what mass of CO₂ is emitted into the atmosphere during the grilling of the pork roast?

Charcoal is primarily carbon. Determine the mass of CO₂ produced by burning enough carbon (in the form of charcoal) to produce 5.00×10² kJ of heat. C(s) + O₂(g) → CO₂(g) ΔH°_rxn = –393.5 kJ