Net Moles of Gas

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ClaireHW
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Net Moles of Gas

Postby ClaireHW » Wed Nov 08, 2017 7:05 pm

Given the balanced equations: 2C4H10 + 13O2 -> 8CO2 + 10H2O
What is the net number of moles of gas produced if 4 moles of C4H10 are used?

(Claire Woolson Dis 3J)

Chem_Mod
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Re: Net Moles of Gas

Postby Chem_Mod » Wed Nov 08, 2017 7:38 pm

Assuming that H2O is a liquid here, we'd use up 26 moles of O2 gas and make 16 moles of CO2. So we have a net loss of 10 moles of gas.

Mitch Walters
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Re: Net Moles of Gas

Postby Mitch Walters » Wed Nov 08, 2017 8:02 pm

Why do we assume that the H2O is a liquid?

ClaireHW
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Re: Net Moles of Gas

Postby ClaireHW » Wed Nov 08, 2017 8:28 pm

The answer given was 6.
I'm wondering how we get to 6 from that amount of moles.

Sabrina Dunbar 1I
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Re: Net Moles of Gas

Postby Sabrina Dunbar 1I » Wed Nov 08, 2017 10:27 pm

Once the equation is balanced, it becomes 4C4H10+26O2-->16CO2+20H20. There are 30 moles of reactants and 36 moles of products. The difference between total moles of products and total moles of reactants gives us the net moles of gas produced (36-30=6). Therefore, the answer is 6 moles of net gas produced by the combustion reaction. We do not assume the H20 is liquid, it should be assumed to be a gas because this is a combustion reaction. Hope this helps!

Golbarg Rahimi 3k
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Re: Net Moles of Gas

Postby Golbarg Rahimi 3k » Wed Nov 08, 2017 10:32 pm

If we have 4 moles of C4H10 that would result in 26 moles o2, 16 moles co2 and 20 moles H2o.
4+26=30
16+20=36
The difference in the gases which is the net gas produced is 36-30=6
In this equation we consider all of the states as gas since the temperature is very high and the water evaporates.


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