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LiRa [457]
3 years ago
8

Which volume of oxygen, at room temperature and pressure, is needed for complete combustion

Chemistry
2 answers:
lesantik [10]3 years ago
6 0
To determine the volume of oxygen needed for the reaction, we need to know the chemical formula of the fuel in order to know the chemical reaction.  Methylpropan-1-ol has a formula of C4H10O. The chemical reaction would be:

C4H10O + 6O2 = 4CO2 + 5H2O

We calculate volume as follows:

1 mol C4H10O ( 6 mol O2 / 1 mol C4H10O) ( 22.4 L O2 / 1 mol O2) = 134.4 L O2 needed or 134.4 dm^3

Therefore, the closest value would be B, 144 dm^3.
adell [148]3 years ago
5 0
The molecular formula of methylpropan-1-ol is C4H10O, so the complete combustion equation is: C4H10O + 6O2 --> 4CO2 + 5H2O.  This mean to completely combust 1.0mol of methylpropan-1-ol, 6 mol of O2 is required. Molar mass of O2 is 32 g/mol, so 32g/mol x 6mol = 192 g of O2 is required.  At room temperature and pressure, the density of O2 is 1.3315 g/L (this can be obtained by density of gas = P/RT).  So the volume of O2 = mass/density = 192g/1.3315(g/L) = 144 L = 144 dm3. The answer is B.
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The Reaction is spontaneous when temperature is 430 K. Hence, Option (C) is correct.

<h3></h3><h3>What is Spontaneous reaction ?</h3>

Reactions are favorable when they result in a decrease in enthalpy and an increase in entropy of the system.

When both of these conditions are met, the reaction occurs naturally.

Spontaneous reaction is a reaction that favors the formation of products at the conditions under which the reaction is occurring.

According to Gibb's equation:

ΔG = ΔH - TΔS

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ΔH = enthalpy change  = +62.4 kJ/mol

ΔS = entropy change  = +0.145 kJ/molK

T = temperature in Kelvin

  • ΔG  = +ve, reaction is non spontaneous
  • ΔG = -ve, reaction is spontaneous
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ΔH - TΔS = 0 for reaction to be spontaneous

T = ΔH / ΔS

Here,

T = 500K

Thus the Reaction is spontaneous when temperature is 500 K.

Learn more about Gibbs free energy here ;

https://brainly.in/question/13372282

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