The combustion of methane gas, the principal constituent of natural gas, is represented by the equation 

(a) What mass of methane, in kilograms, must be burned to liberate 2.80 x 107 kJ of heat?

(b) What quantity of heat, in kilojoules, is liberated in the complete combustion of 1.65 x 104 L of CH₄(g), measured at 18.6 °C and 768 mmHg?

(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 8.8 to 60.0 °C as a result?

Transcribed Image Text:

CH4(g) + 2O2(g) CO₂(g) + 2H₂O(1) A,H° -890.3 kJ mol-1 =