This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Hey yakubutimjul, good to see you again. Step 1: Write the balanced chemical equation for the decomposition of N₂O₅. The decomposition of dinitrogen pentoxide (N₂O₅) produces nitrogen dioxide (NO₂) and oxygen (O₂). 2 N_2O_5(g) → 4 NO_2(g) + O_2(g) Step 2: Calculate the moles of O₂ produced. At Standard Temperature and Pressure (STP), 1 mole of any gas occupies 22.4 litres. Given volume of O₂ = 2.24 litres. Moles of O_2 = Volume of O_2Molar volume at STP Moles of O_2 = 2.24 L22.4 L/mol Moles of O_2 = 0.1 mol Step 3: Calculate the rate of production of O₂. The time taken is 30 minutes. Rate of O_2 production = Moles of O_2Time Rate of O_2 production = 0.1 mol30 min Rate of O_2 production = 0.00333 mol/min Step 4: Determine the rate of disappearance of N₂O₅ using stoichiometry. From the balanced equation, 2 moles of N₂O₅ decompose for every 1 mole of O₂ produced. Rate of disappearance of N_2O_5 = 2 × Rate of O_2 production Rate of disappearance of N_2O_5 = 2 × 0.00333 mol/min Rate of disappearance of N_2O_5 = 0.00666 mol/min The rate of disappearance of N₂O₅ is: 0.00666 mol/min Send me the next one 📸