The combustion of methane gas, the principle component of natural gas, is repres
ID: 951487 • Letter: T
Question
The combustion of methane gas, the principle component of natural gas, is represented by the equation CH_4 (g) + 2 O_2 (g) rightarrow CO_2 (g) + 2 H_2 O (I) Delta H = -890.3 kJ What mass of methane, in kg must be burned to liberate 1.00 Times 10^6 kJ of heat? If the quantity of heat stated in part (a) could be transferred with 100 % efficiency to water, what volume of water, in L, could be heated from 22.7 degree C to 60.8 degree C as a result? (After gases) What quantity of heat, in kJ, is liberated in the complete combustion of 1.03 Times 10^3 L of CH_4 (g) measured at 21.8 degree C and 748 mmHg?Explanation / Answer
Solution:
a) The thermodynamic for mass calculation is by,
q = del H = mCp(T2-T1)
-890.3 = m (2.26) (25)
m = 15.75 kg for 1kJ so for 1.00E6 kJ the total mass required is,
m = 15.75 E6 kg
b) by using boyles law PV = RT,
V = (T2/T1) * V1
= (60.8 / 22.7) * 15.75 E6
= 42.18 E6 Lt
c) by using q equation mentioned in (a) we get,
q = del H = mCp(T2-T1)
q = 1.03 E3 * 2.26 * (25 - 21.8)
q = 7.232 E3 kJ of heat liberated