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if 5.8 moles of nitrogen monoxide (no) react with 10.0 moles of oxygen gas (o2), how many moles of the product can be formed and how many moles of the excess reactant will be left over when the reaction is complete? show all of your work.

unbalanced equation: no + o2 --> no2

The balanced chemical equation would be as follows:

2NO + O2 --> 2NO2

We are given the amount of reactants to be used for the reaction. We use these amounts to determine first which is the limiting reactant. The ratio of the reactants from the reaction is 2:1. Therefore, the limiting reactant would be nitrogen monoxide since it can be consumed completely. Calculations are as follows:

5.8 mol NO ( 2 mol NO2 / 2 mol NO ) = 5.8 mol NO2 is produced
10.0 mol O2 - (5.8 mol NO) ( 1 mol O2 / 2 mol NO ) = 7.1 mol O2 excess.

This is what i found on google “when one phosphate group is removed by breaking a phosphoanhydride bond in a process called hydrolysis, energy is released, and atp is converted to adenosine diphosphate (adp). likewise, energy is also released when a phosphate is removed from adp to form adenosine monophosphate (amp).” i hope this you .

What do you need with it’s not a question your just stating what it says