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sineoko [7]
3 years ago
6

(6.21×10^3)(0.1050) (Scientific Notation)

Chemistry
1 answer:
mel-nik [20]3 years ago
3 0
6.21 x 10^3 = (Move decimal point 3 spaces to the right)

6210

6210 (0.1050)

652.05
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Use bond energies to calculate the enthalpy of reaction for the combustion of ethane. Average bond energies in kJ/mol C-C 347, C
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The enthalpy of reaction for the combustion of ethane 2CH₃CH₃ + 7O₂ → 4CO₂ + 6H₂O calculated from the average bond energies of the compounds is -2860 kJ/mol.

The reaction is:

2CH₃CH₃ + 7O₂ → 4CO₂ + 6H₂O  (1)  

The enthalpy of reaction (1) is given by:

\Delta H = \Delta H_{r} - \Delta H_{p}   (2)

Where:

r: is for reactants

p: is for products

The bonds of the compounds of reaction (1) are:

  • 2CH₃CH₃: 2 moles of 6 C-H bonds + 2 moles of 1 C-C bond
  • 7O₂: 7 moles of 1 O=O bond  
  • 4CO₂: 4 moles of 2 C=O bonds  
  • 6H₂O: 6 moles of 2 H-O bonds

Hence, the enthalpy of reaction (1) is (eq 2):

\Delta H = \Delta H_{r} - \Delta H_{p}

\Delta H = 2*\Delta H_{CH_{3}CH_{3}} + 7\Delta H_{O_{2}} - (4*\Delta H_{CO_{2}} + 6*\Delta H_{H_{2}O})      

\Delta H = 2*(6*\Delta H_{C-H} + \Delta H_{C-C}) + 7\Delta H_{O=O} - (4*2*\Delta H_{C=O} + 6*2*\Delta H_{H-O})  

\Delta H = [2*(6*413 + 347) + 7*498 - (4*2*799 + 6*2*467)] kJ/mol  

\Delta H = -2860 kJ/mol          

Therefore, the enthalpy of reaction for the combustion of ethane is -2860 kJ/mol.

Read more here:

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A compound with the formula C6H14 was reacted with Cl2/light to give a mixture of 5 different monochlorinated products (not incl
allochka39001 [22]

Answer:

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Explanation:

Hello!

In this case, since the general reaction of the compound C4H14 with chlorine is:

C_6H_{14}+Cl_2\rightarrow C_6H_{13}Cl+HCl

Which stands for a substitution chemical reaction in which one chlorine is able to replace one hydrogen and therefore hydrogen chloride gives off; we infer that the initial compound, C4H14, shows off the C_nH_{2n+2} formula characteristic of alkanes; in such a way, as it has six carbon atoms, we infer it is hexane.

Best regards!

6 0
3 years ago
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