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May 23rd, 2018, 11:38 AM   #1
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Calculate Energy Required OR Released

Calculate the amount of energy required or released in the formation reaction for five moles of liquid water H2O(l). This occurs at standard temperature and pressure. Express your answer in joules. The heat of formation of water is -285.8 kJ/mol. Is this an endothermic or exothermic reaction? Explain your reasoning and show all your work to receive full credit.

Could anyone point me in the right direction with this? I am going back through my chemistry lessons but really have no idea where to begin with this. Any help will be greatly appreciated! Thanks.
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May 23rd, 2018, 03:03 PM   #2
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It's exothermic, as the heat of formation is negative.
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May 23rd, 2018, 05:43 PM   #3
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So if it's exothermic, heat is released... which means that is what needs calculated, the amount of heat released. How could I begin to set this equation up?
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May 23rd, 2018, 10:39 PM   #4
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The heat released is 285.8 kJ/mol, so multiply that by 5 mol.
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