8. Ammonia reacts with oxygen to produce nitrogen monoxide ar water according to the following chemical reaction. 4NH_(3)(g)+5O_(2)(g)Longrightarrow 4NO(g)+6H_(2)O(l) If 128 g O_(2) reacts with excess NH3 what mass of NO is produced? 3.2 g 96g 120 g 45g

To solve this problem, we need to use the balanced chemical equation and the given information to determine the mass of NO produced.Given information:- The balanced chemical equation is: - 128 g of reacts with excess .Step 1: Calculate the molar mass of .Molar mass of = 32 g/molStep 2: Calculate the number of moles of .Number of moles of = 128 g / 32 g/mol = 4 molStep 3: Use the balanced chemical equation to determine the number of moles of NO produced.According to the balanced equation, 5 moles of produce 4 moles of NO.Number of moles of NO produced = (4 mol ) × (4 mol NO / 5 mol ) = 3.2 mol NOStep 4: Calculate the mass of NO produced.Molar mass of NO = 30 g/molMass of NO produced = 3.2 mol × 30 g/mol = 96 gTherefore, the correct answer is 96 g.