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

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