If 6.2 moles of nitrogen monoxide (NO) react with 13.0 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

Question

If 6.2 moles of nitrogen monoxide (NO) react with 13.0 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

anonymous · Answer

2NO + O2 ---> 2NO2

anonymous · Answer

balanced equation ^

anonymous · Answer

are you doing flvs?

anonymous · Answer

yes module 4 i dont get this question

anonymous · Answer

no way im doing the same module um what test ive already taken all mine, but i skipped the module test so im taking that now. but maybe i can help you out?

anonymous · Answer

yes please!

anonymous · Answer

i just have 3 more questions and im done

anonymous · Answer

okay hey maybe you can help me out with my last question too

anonymous · Answer

totally

anonymous · Answer

okay what are your last 3 questions?

anonymous · Answer

but first what test are you taking in module 4?

anonymous · Answer

the last one honors

anonymous · Answer

okay what are the questions?

anonymous · Answer

If 5.85 grams of cobalt metal react with 15.8 grams of silver nitrate, how many grams of silver metal can be formed and how many grams of the excess reactant will be left over when the reaction is complete? Show all of your work.

unbalanced equation: Co + AgNO3   Co(NO3)2 + Ag

anonymous · Answer

if 6.2 moles of nitrogen monoxide (NO) react with 13.0 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

anonymous · Answer

thats it i just finished the other one

anonymous · Answer

its been answered on yahoo answers

anonymous · Answer

i dont get the second one though the answer is weird

anonymous · Answer

hmm i dont know, im struggling with the same thing on my test to

anonymous · Answer

are you taking semester 2?

anonymous · Answer

yeah oh hey i found out how to solve your problem Steps to solving it:
1) Identify limiting reagent
2) Use sample of limiting reagent to calculate expected Fe yield.
3) Divide theoretical yield by expected yield to get the percent yield.

anonymous · Answer

finished that one haha thanks though! but we should help each other on the second semester

anonymous · Answer

for sure