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satela [25.4K]
3 years ago
7

When a 3.80 g sample of liquid octane (c8h18) is burned in a bomb calorimeter, the temperature of the calorimeter rises by 27.3

∘c. the heat capacity of the calorimeter, measured in a separate experiment, is 6.10 kj/∘c . determine δerxn for the combustion of octane in units of kj/mol octane?
Chemistry
1 answer:
photoshop1234 [79]3 years ago
5 0

Δerxn  for  the combustion  of octate   in   kj/mol  is  4995.48  kj/mol


<u><em>calculation</em></u>

Step  1 :  calculate Δ T

ΔH  =  CΔT  where

 C=  specific heat capacity= 6.10 kj/°c

ΔT = change in temperature =  27.3 °c

ΔH  is  therefore =  27.3 °c  x  6.10  kj/°c  =166.53  kj


Step 2:  calculate ΔH   per  gram

ΔH   per  gram   of the sample=   166.53 kj/ 3.80 g  = 43.82  kj/g


Step: calculate ΔH  erxn  in  kj/mol

Δ H erxn  in kj /mol   =  43.82  x molar mass of C8H18The molar mass  of C8H18  is =  (12  x8)  +( 1 x18)  =  114 g/mol

Δ erxn is  therefore  = 43.82  kj/g  x 114  g/mol = 4995.48 kj/mol


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Explanation:

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T = Temperature of the gas = 25^oC=[25+273]K=298K

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Putting values in above equation, we get:

805torr\times 0.235L=n\times 62.3637\text{ torrHg }mol^{-1}K^{-1}\times 298K\\\\n=\frac{805\times 0.235}{62.3637\times 298}=0.01017\ mol

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1 mole of chlorine gas is produced when 1 mole of manganese dioxide undergoes reaction.

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0.01017 mole of chlorine gas is produced when 0.01017 mole of manganese dioxide undergoes reaction.

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Mass=Moles\times Molar\ mass

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