You need more information to answer the next two, as … And the answer would be 4.78 x 4/5 or 3.824 moles of NO. Which reactant is the limiting reagent?… A) 5 moles of O2 produce 4 moles of NO. Solution for Take the reaction: NH3+O2-> NO+H2O. So the molar ration is 5 to 4. A. Take the reaction: NH3 + O2 + NO + H2O. 160.00 g of O2 / g/mol for O2 = number of moles of O2. First you have to balance the reaction to determine the mole ratios of the reactants and products. 8.0 moles * 30.01 g/mol = 240.08 grams of Nitric oxide. In an experiment, 3.25g of NH3 are allowed - 16235523 Problem: NH3 + O2 → NO + H2O (Unbalanced)If at the beginning of the reaction you used 6.89 g NH3 and 15.76 g O2, what is the theoretical yield (in grams) of NO (you will need to find the limiting reagent and then the theoretical yield of NO from this reagent)? For the reaction NH3 + O2 --> NO + H2O how many grams of O2 are needed to completely react with 85.15 g of NH3 ? Remember the moles of the unknown is in the numerator. Molar Mass:… Identify the type of reaction NH3+O2---> NO + H2O 1 See answer apoorvavishwasr4476 is waiting for your help. The first thing you need is a balanced equation for the reaction: 4 NH3 + 5 O2 → 4 NO + 6 H2O. 1. Still have questions? The balanced reaction is: 4NH3 + 5O2 --> 4NO + 6H2O. Solution for Consider the reaction: NH3 + O2 → NO + H2O For every 150 g NH3, Find the mass of NO produced. Ask your question. Add your answer and earn points. ash1719 ash1719 Redox and neutralization reaction Still have questions? Find the mass of H2O produced. In an experiment 3.25g of NH3 are allowed to react with 3.50g of O2. So the conversion factor would be 4/5. Both of them limit the Hydrogen. Limiting reactant is Nitrogen and Oxygen, by just giving it a quick look. This would produce 8.0 moles of NO. Find more answers. 160.00 g / 16.00 g/mol = 10.0 moles of O2.

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