Question

part B and D???

Review I Constants Learning Goal: Correct To understand how to use stoichiometry to convert between quantities of reactants and products in chemical equations. Stoichiometry describes the quantitative relationships among the reactants and products of a balanced reaction by directly comparing mole ratios. Stoichiometry can be used to convert mass, number of moles, or number of particles between products and reactants, as shown in the flowchart displayed in the figure. (Figure 1) Part B How many grams of NHs can be produced from 4.22 mol of N2 and excess H2. Express your answer numerically in grams. View Available Hint(s) Figure V AX ? 1 of 1 g NH number of particles mass Substance A Avogadro's nuinber molar mass Submit Previous Answers moles oefficients from balanced chemical equation X Incorrect; Try Again; 4 attempts remaining moles Avogadro's mumber molar mass Substance B Part C number of partides mass How many grams of H, are needed to produce 14.90 g of NH,? Express your answer numerically in grams. MacBook Air

Answer 1

N₂ + 3H₂2NH3 mol of N₂ = 4.22 mol mol of Ny gives 2 mol of NH3 4.22 mol of N₂ = 2x4.22 = 8.44 mol of NH3 molar mass of NH3 = 17.03g1 ma mass of NH3 produced - 8.44817.03 = 143.73g mass of H2 = 6.32x 10-4 g moles of H₂ z 6.328104 g 2g/mol = 3.16 x 10-4 mol and of H2 2 nd og NH3 moles of NH3 produced 8x3.16x10 mol - 2.106 8 10 a moles no. of molecules = 2.106810-4x6.022x10 23 = 12.6868 1019 molecules