Net Moles Produced  [ENDORSED]

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isauramora3K
Posts: 20
Joined: Fri Sep 29, 2017 7:07 am

Net Moles Produced

Postby isauramora3K » Fri Oct 06, 2017 10:20 pm

What does it mean when it asks for net number of moles produced?

Curtis Wong 2D
Posts: 62
Joined: Sat Jul 22, 2017 3:00 am

Re: Net Moles Produced

Postby Curtis Wong 2D » Fri Oct 06, 2017 10:27 pm

It just basically asks for how much the equation produced. If it's using the number of moles of equation, then it's how many gets produced in the equation (ie 1H2O -> 2 moles of H and 1 mole of O, giving 3 moles produced). If it's using an amount of moles, then you have to figure out the ratios first before answering the question

Eli Aminpour 2K
Posts: 50
Joined: Fri Sep 29, 2017 7:04 am

Re: Net Moles Produced

Postby Eli Aminpour 2K » Fri Oct 06, 2017 11:15 pm

A trick to problems like these is to add the coefficients of the reactants and subtract that value from the sum of the coefficients of products. Make sure to balance the chemical equation first

Karan Singh Lecture 3
Posts: 23
Joined: Fri Sep 29, 2017 7:07 am

Re: Net Moles Produced  [ENDORSED]

Postby Karan Singh Lecture 3 » Sat Oct 07, 2017 1:03 am

All you do is count up the moles of the products and subtract by the moles of the reactants and that is your net moles.

Ashley Davis 1I
Posts: 57
Joined: Fri Sep 29, 2017 7:04 am

Re: Net Moles Produced

Postby Ashley Davis 1I » Sat Oct 07, 2017 10:30 am

Add the coefficients of the reactants together and then subtract the sum of the coefficients of the products from that. For example, if the reaction were 2K + 10W --> 5L + 4R, then the net moles produced would be 12 - 9 = 3 net moles.

Ruohan Sun 3I
Posts: 19
Joined: Fri Sep 29, 2017 7:07 am

Re: Net Moles Produced

Postby Ruohan Sun 3I » Sat Oct 07, 2017 4:15 pm

just subtract the coefficients of products by the coefficients of reactants


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