# nh3+o2=no+h2o type of reaction

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

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