How many moles of H2o are required to produce 4.5 moles of HNo3, according to the following reaction 3No2+H2o=2HNo3+No
According to the balanced chemical equation, the stoichiometry is as follows:
3 NO2 + H2O → 2 HNO3 + NO
From the equation, we can see that 3 moles of NO2 produces 2 moles of HNO3.
So, for every 1 mole of HNO3 produced, 3/2 moles of NO2 are required.
Therefore, for 4.5 moles of HNO3, the number of moles of NO2 required would be (4.5 mol HNO3) x (3/2 mol NO2/1 mol HNO3) = 6.75 mol NO2.
However, the question asks for the number of moles of H2O required, not NO2.
From the equation, we can see that 1 mole of H2O reacts with 2 moles of HNO3.
So, for every 2 moles of HNO3 produced, 1 mole of H2O is required.
Therefore, for 4.5 moles of HNO3, the number of moles of H2O required would be (4.5 mol HNO3) x (1 mol H2O/2 mol HNO3) = 2.25 mol H2O.
Therefore, 2.25 moles of H2O are required to produce 4.5 moles of HNO3.