chemistry question

Question

1. Chemistry mixes 108 g of H2O, with 186 L of NO2 at STP. How many grams of NO will be produced? The balanced equation for this reaction is:

H2O + 3 NO2 🡪 2 HNO3 + NO

Answer 1

It's a limiting reactant problem. Compare the moles of each reactant to the stoichiometric mix of NO₂/H₂O of 3/1:

108 g H₂O (1 mole/18.02g H₂O) = 5.99 moles water

186 L NO₂ (1 mole/22.4 L @STP) = 8.30 moles NO₂ (LR as you need 3x the water moles)

Now, just continue stoichiometric calculation using the LR:

8.30 moles NO₂ (1 NO/3 NO₂)( 30.01 g/mole NO) = g of NO

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