A rigid vessel holds 1.00 mol of N₂ and 2.00 mol of H₂. The reaction N₂ + 3 H₂ → 2 NH₃ proceeds until 30% of the nitrogen has been used. What is the average molar mass of the gas mixture then? Atomic masses in g mol⁻¹: H 1.0, N 14.0.

ChemistryAdvancedHigh School (11–12)Atoms and Molecules › The Mole Concept Olympiad

A rigid vessel holds $1.00\ \text{mol}$ of $\text{N}_2$ and $2.00\ \text{mol}$ of $\text{H}_2$ . The reaction $\text{N}_2 + 3\,\text{H}_2 \rightarrow 2\,\text{NH}_3$ proceeds until $30\%$ of the nitrogen has been used. What is the average molar mass of the gas mixture then? Atomic masses in $\text{g mol}^{-1}$ : H 1.0, N 14.0.

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← A metal M of mass 0.600 g dissolves in dilute acid and gives 0.560 L of hydrogen at STP, where 11.2 L of hydrogen is one equivalent. The vapour density of the metal chloride, relative to hydrogen, is 47.5. What is the atomic mass of M? Atomic masses in g mol⁻¹: Cl 35.5.A solution contains oxalic acid, H₂C₂O₄, and sodium hydrogen oxalate, NaHC₂O₄. A 25.0 mL portion needs 20.0 mL of 0.100 mol L⁻¹ NaOH to reach the phenolphthalein end point. A second 25.0 mL portion, in acid, needs 16.0 mL of 0.0400 mol L⁻¹ KMnO₄, where 2 MnO₄⁻ + 5 C₂O₄²⁻ + 16 H⁺ → 2 Mn²⁺ + 10 CO₂ + 8 H₂O. What is the molarity of NaHC₂O₄ in the solution? →

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