The combustion of methane gas, the principal constituent of natural gas, is represented by the equation
CH4 + 2O2-->CO2+H2O Change in H is -890.3kJ
a What mass of methane, in kilograms, must be burned to liberate 2.00×10^7 of heat?
b What quantity of heat, in kilojoules, is liberated in the complete combustion of 1.55×10^4 L of CH4, measured at 18.4 degrees C and 774mmHg?
c. If the quantity of heat calculated in part (b) could be transferred with 100% efficiency to water, what volume of water, in liters, could be heated from 8.6 to 60.0 degrees C as a result?