boSuppose a boil water notice is sent out advising all residents in the area to boil their water before drinking it or using it for cooking. You need to boil 11.5 L of water using your natural gas (primarily methane) stove. What volume of natural gas is needed to boil the water if only 19.3% of the heat generated goes towards heating the water. Assume the density of methane is Macmillan Learning 0.668 g/L, the density of water is 1.00 g/mL, and that the water has an initial temperature of 20.8 °C. Enthalpy of formation values can be found in this table. Assume that gaseous water is formed in the combustion of methane. volume of methane: x10 TOOLS L

If 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?

You heat 1.000 quart of water from 25.0C to its normal boiling point by burning a quantity of methane gas, CH4. What volume of methane at 23.0C and 745 mmHg would you require to heat this quantity of water, assuming that the methane is completely burned? The products are liquid water and gaseous carbon dioxide.

A rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.