Chemistry Question: need help with this?
One of the steps in commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO:
4NH3(g) + 5O2(g) --> 4NO9g) + 6H2O
In a certain experiment, 2.25g og NH3 react with 3.75g of O2
(a) which is the limiting reactant?
(b) How many grams of NO form?
Answer:
I'll get you started. You need to convert the grams to moles for both NH3 and 02. Whichever has the smallest number of moles will be your limiting reagent. (hint: NH3 has a molecular weight of 17.04 g/mol, O2 has 32.00 g/mol)
Once you find your limiting reagent (hint: you will calculate that it has 0.12 mol if you're doing everything right), you can calculate the moles of NO formed--don't forget to take into account the ratio of moles of limiting reagent to moles of reactant.
Once you have the moles of NO, use NO's molecular weight to calculate the grams of NO formed.
You'll learn a lot more if you do the math yourself, so I only wanted to give you a guide. I know chemistry can be challenging at first, but keep practicing! You will succeed.
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4NH3(g) + 5O2(g) --> 4NO9g) + 6H2O
In a certain experiment, 2.25g og NH3 react with 3.75g of O2
(a) which is the limiting reactant?
(b) How many grams of NO form?
Answer:
I'll get you started. You need to convert the grams to moles for both NH3 and 02. Whichever has the smallest number of moles will be your limiting reagent. (hint: NH3 has a molecular weight of 17.04 g/mol, O2 has 32.00 g/mol)
Once you find your limiting reagent (hint: you will calculate that it has 0.12 mol if you're doing everything right), you can calculate the moles of NO formed--don't forget to take into account the ratio of moles of limiting reagent to moles of reactant.
Once you have the moles of NO, use NO's molecular weight to calculate the grams of NO formed.
You'll learn a lot more if you do the math yourself, so I only wanted to give you a guide. I know chemistry can be challenging at first, but keep practicing! You will succeed.
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