Propane (C₃H₈) is one of the gases that is used as fuel gas. Propane has a normal boiling point of –42.0°C and its enthalpy of vaporization is 14.79 kJ/mol. Calculate the heat that must be added to convert 300 g of propane into vapor and determine the volume of this propane gas occupies at 765 torr and 40.0°C.

If the energy from the reaction of HNO₂ shown below is used to create NO₂, how many moles of NO₂ can be created per mole of HNO₂? The energy needed to create 1.00 mol of NO₂ is  122.92 kJ.

Calculate the mass of CO₂ emitted by the combustion of pentane (C₅H₁₂) to generate 5.96 x 10² kJ of heat. The balanced reaction is shown below:

C₅H₁₂(g) + 8 O₂(g) → 5 CO₂(g) + 6 H₂O(l) ΔH°_rxn = –3509 kJ

Butane (C₄H₁₀) used in a grill burns according to the following reaction: 

2 C₄H₁₀( g) + 13 O₂(g) → 8 CO₂(g) + 10 H₂O(g) ΔH°_rxn = -5756.6 kJ 

A certain piece of steak needs to absorb 539 kJ to fully cook. Calculate the mass of CO₂ emitted if only 15% of the heat produced is actually absorbed by the steak.

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 x 10³ kJ to be fully cooked, and if only 10% of the heat produced by the barbeque is 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