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Lemonadestars
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2-methylpropene can be obtained by dehydrating 2-methylpropan-1-ol.
(CH3)2CHCH2OH(l) →*(CH3)2C=CH2(g) + H2O(l)
The standard enthalpies of formation of 2-methylpropan-1-ol, 2-methylpropene and water are −335, −17 and −286 kJ mol−1*respectively.
What is the standard enthalpy change for the dehydration of 2-methylpropan-1-ol?
Idk did I done it right, I was thinking since the 2-methylpropan-1-ol did not shows up as a final product, so only add up heat of 2-methylpropan-1-ol and water, is it the right answer?
(CH3)2CHCH2OH(l) →*(CH3)2C=CH2(g) + H2O(l)
The standard enthalpies of formation of 2-methylpropan-1-ol, 2-methylpropene and water are −335, −17 and −286 kJ mol−1*respectively.
What is the standard enthalpy change for the dehydration of 2-methylpropan-1-ol?
Idk did I done it right, I was thinking since the 2-methylpropan-1-ol did not shows up as a final product, so only add up heat of 2-methylpropan-1-ol and water, is it the right answer?
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bl0bf1sh
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with these kinds of questions, what do you normally need to do if you are given values for standard enthalpies of formation?
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hint
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can you draw a Hess cycle?
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remember the definition of "standard enthalpy of formation" – you need to make sure you use the right numbers
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Lemonadestars
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Ty! I tried to calculate it, since formation of water have same enthalpy as these two adds up, so the equation should be -286-(-335-17)=66kJ/mol, is it the right answer?
(Original post by bl0bf1sh)
with these kinds of questions, what do you normally need to do if you are given values for standard enthalpies of formation?
with these kinds of questions, what do you normally need to do if you are given values for standard enthalpies of formation?
Spoiler:
Show
hint
Spoiler:
Show
can you draw a Hess cycle?
Spoiler:
Show
remember the definition of "standard enthalpy of formation" – you need to make sure you use the right numbers
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bl0bf1sh
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not quite sure what you mean by "formation of water have same enthalpy as these two adds up"?
I got a different value
have you drawn a Hess cycle? are your arrows pointing in the right direction? are you changing the sign (+/-) if you are going the opposite way to the direction of the arrow?
handy page on Hess cycles: https://chemguide.co.uk/physical/energetics/sums.html
I got a different value
have you drawn a Hess cycle? are your arrows pointing in the right direction? are you changing the sign (+/-) if you are going the opposite way to the direction of the arrow?
handy page on Hess cycles: https://chemguide.co.uk/physical/energetics/sums.html
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charco
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(Original post by Lemonadestars)
2-methylpropene can be obtained by dehydrating 2-methylpropan-1-ol.
(CH3)2CHCH2OH(l) →*(CH3)2C=CH2(g) + H2O(l)
The standard enthalpies of formation of 2-methylpropan-1-ol, 2-methylpropene and water are −335, −17 and −286 kJ mol−1*respectively.
What is the standard enthalpy change for the dehydration of 2-methylpropan-1-ol?
Idk did I done it right, I was thinking since the 2-methylpropan-1-ol did not shows up as a final product, so only add up heat of 2-methylpropan-1-ol and water, is it the right answer?
2-methylpropene can be obtained by dehydrating 2-methylpropan-1-ol.
(CH3)2CHCH2OH(l) →*(CH3)2C=CH2(g) + H2O(l)
The standard enthalpies of formation of 2-methylpropan-1-ol, 2-methylpropene and water are −335, −17 and −286 kJ mol−1*respectively.
What is the standard enthalpy change for the dehydration of 2-methylpropan-1-ol?
Idk did I done it right, I was thinking since the 2-methylpropan-1-ol did not shows up as a final product, so only add up heat of 2-methylpropan-1-ol and water, is it the right answer?
Here is a video that shows you how to apply enthalpy changes to determine reaction enthalpy.
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