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Lena [83]
2 years ago
5

Hi friends!!!!!!!!!!!​

Chemistry
2 answers:
vodka [1.7K]2 years ago
6 0

Answer:

yo hi grand how it go nice guy

Anna11 [10]2 years ago
5 0

Answer:

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Use bond energies from Table 10.3 in the textbook to estimate the enthalpy change (ΔH) for the following reaction. C2H2(g)+H2(g)
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Answer: =176.6kJmol^{-1}

Explanation:Bond energy of H-H is 436.4 kJ/mole

Bond energy of  C-H is 414 kJ/mol

Bond energy of C=C is 620 kJ/mol

Bond energy of C≡C is 835 kJ/mol

\Delta H= {\text {sum of bond energies of reactants}}-  {\text {sum of bond energies of products}}

\Delta H= {1B.E(C≡C)+2B.E(C-H) +1B.E(H-H)} - {1B.E(C=C)+4B.E(C-H)}

\Delta H= {1B.E(835kJmole^{-1})+2B.E(414kJmole^{-1}) +1B.E(436.4kJmole^{-1})} -  {1B.E(620kJmole^{-1})+4B.E(414kjmole^{-1})}

=176.6kJmol^{-1}







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What can be expected to occur as climate change continues on earth?
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Keera decided to investigate how the growth of plants is affected by the time of day it is watered. She placed an equal amount o
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