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Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation: Na(g) + 3H2(g) → 2NH3(0) 1. What is the maximum mass of ammonia that can be produced from a mixture of 131.5 g of N₂ and 32.36 g of H₂? 2. Which element would be left partially unreacted? (enter nitrogen or hydrogen) 3. What mass of the starting material would remain unreacted?

A compound contains only carbon, hydrogen, and oxygen. Combustion of 30.63 g of the compound yields 44.89 g of CO2 and 18.38 g of H₂0. The molar mass of the compound is 180.156 g/mol. *Each part of this problem should be submitted separately to avoid losing your work 1. Calculate the grams of carbon (C) in 30.63 g of the compound: 12.25 grams 2. Calculate the grams of hydrogen (H) in 30.63 g of the compound. 2.056 grams 3. Calculate the grams of oxygen (0) in 30.63 g of the compound. 16.32 grams You are correct. Previous Tries Based on your previous answers, calculate 1. the moles of carbon (C) in 30.63 g of the compound: 1021 2. the moles of hydrogen (H) in 30.63 g of the compound: 1021 3. the moles of oxygen (0) in 30.63 g of the compound: 1.021 moles moles moles Use the molar mass given on the periodic table for O,H and C to find the number of moles of each. Your answers should follow the sig fig rules and use your correct answers from the previous problem to do these calculations. Submit Answer Incorrect Tries 1/10 Previous Tries Divide each mole quantity that you determined in the previous question by the smallest number of moles to determine the correct empirical formula. Enter the correct subscript for each atom using the smallest whole number. Enter a 1 if that is the smallest whole number, don't leave the box empty. Ce He 06 Remember, after you divide by the smallest number of moles, if one (or more) of the numbers is a fraction, multiply all mole quantities by a factor that will give the smallest whole number values. Submit Answer Incorrect. Tries 1/10 Previous Tries Po Boss Bi Now determine the molecular formula. Remember that the molar mass of the compound is 180.156 g/mol. Enter the correct subscript for each atom using the smallest whole number. Enter a 1 if that is the smallest whole number, don't leave the box empty. C H O Submit Answer Tries 0/10