If you attempt to produce work using the formation reaction of methanol (CH3OH), and the reaction is carried out reversibly, wha
1 answer:
The minimum amount of heat wasted in the production of methanol is 239kJ/mol of heat.
<h3>What is the heat wasted?</h3>Now we know that the enthalpy is the heat that is released or absorbed in a reaction. The reaction involves the combination of reactants that leads to the formation of the product(s).
Now we know that the production of methanol leads to the evolution of about 239kJ/mol of heat. This heat is wasted as it goes to no good use but is just lost to the environment.
As such, the minimum amount of heat wasted in the production of methanol is 239kJ/mol of heat.
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Answer: Option (b) is the correct answer.
Explanation:
A covalent bond is defined as the bond which occurs due to sharing of electrons between the combining atoms.
Generally, a covalent bond is formed between non-metals.
For example, both nitrogen and oxygen atoms are non-metals and they combine covalently to form compound.
As nitrogen has 5 valence electrons and an oxygen atom has 6 valence electrons. So, there occurs unequal sharing of electrons between the two.
Thus, we can conclude that when a covalent bond forms then electrons in valence shells are shared between atoms.
Answer : The correct option is, (D) 3600 kJ
Explanation :
Mass of octane = 75 g
Molar mass of octane = 114.23 g/mole
Enthalpy of combustion = -5500 kJ/mol
First we have to calculate the moles of octane.
Now we have to calculate the heat released in the reaction.
As, 1 mole of octane released heat = -5500 kJ
So, 0.656 mole of octane released heat = 0.656 × (-5500 kJ)
= -3608 kJ
≈ -3600 kJ
Therefore, the heat released in the reaction is 3600 kJ