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

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