The heats of reaction for the combustion of CH4, and H2 are given below CH_4 +20
ID: 924385 • Letter: T
Question
The heats of reaction for the combustion of CH4, and H2 are given below CH_4 +202 rightarrow CO_2+ 2H_20 deltaHrxn = -802.3kJ H_2 + Vi 02 rightarrow H20 deltaHfxn = -241.8kJ Using the values for the bond enthalpies given in the table below to determine the amount of energy given off when acetylene, C_2H_2, burns as shown below. (Acetylene is a gas used in welding.) 2 C_2H_2 (g) + 5 02 (g) rightarrow 4 C0_2 (g) + 2 H_20(g) Is there more or less heat released for acetylene compared to CH_4? The fuel value is the energy released per gram of substance. What is the fuel value of the three fuels (acetylene, methane and hydrogen)? Which of the three has the greatest fuel value? The energy density (energy released per unit volume) of gasoline is approximately 35 MJ/L (= 35 times 103 kJ/L). Which of the fuels above (CH_4, H_2 or acetylene) has a greater energy density than gasoline? The densities of liquid acetylene, methane and hydrogen are given in the table below. Note these fuels are gases at room temperature: they have to be compressed to get them into the liquid phase. A high energy density means that more energy can be stored in the similar volume (i.e., gas tank).Explanation / Answer
The heats of reaction for the combustion of CH4, and H2 are given below CH_4 +20
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