The combustion of methane gas, the principal constituent of natural gas, is repr

Question

The combustion of methane gas, the principal constituent of natural gas, is represented by the equation
CH4(g)+2O2(g)CO2(g)+2H2O(l)
H=890.3kJ

Part A

What mass of methane, in kilograms, must be burned to liberate 3.40×107 kJ of heat?

Part B

What quantity of heat, in kilojoules, is liberated in the complete combustion of 1.85×104 L of CH4(g), measured at 18.8 C and 774 mmHg ?

Part 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 9.4 to 65.0 C as a result?

The combustion of methane gas, the principal constituent of natural gas, is represented by the equation
CH4(g)+2O2(g)CO2(g)+2H2O(l)
H=890.3kJ

Part A

What mass of methane, in kilograms, must be burned to liberate 3.40×107 kJ of heat?

m = ? kg

Part B

What quantity of heat, in kilojoules, is liberated in the complete combustion of 1.85×104 L of CH4(g), measured at 18.8 C and 774 mmHg ?

|Q| = ? kJ

Part 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 9.4 to 65.0 C as a result?

V = ? L

Explanation / Answer

part A )

CH4 + 2O2 ----------------> CO2 + 2H2O

16g                                             

16g CH4 ----------------> -890.3 kJ

x g CH4   -----------------> 3.40 x 10^7 kJ

x = 16 x 3.40 x 10^7 / 890.3

x = 611030 g

x = 611 kg

mass of CH4 = 611 kg

note : you cropped some data form part b and part c . upload them as soon as

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