Answer: Actual mass of C₉H₈O₄ = (Assumed yield) × (Mass of C₉H₈O₄)
= (0.
Step-by-step explanation:
Let's solve each problem step by step:
To determine the number of moles of O₂ required to generate 13.0 mol of NO₂, we need to use the stoichiometric ratio from the balanced equation:
2 NO (g) + O₂ (g) → 2 NO₂ (g)
From the equation, we can see that the mole ratio between O₂ and NO₂ is 1:2.
Given:
Number of moles of NO₂ = 13.0 mol
To find the moles of O₂, we use the equation:
Moles of O₂ = (Number of moles of NO₂) / 2
Moles of O₂ = 13.0 mol / 2
Moles of O₂ = 6.5 mol
Therefore, 6.5 moles of O₂ would be required to generate 13.0 mol of NO₂.
To calculate the mass of aspirin (C₉H₈O₄) produced from 52.1 g of C₇H₆O₃, assuming a 95.0% yield, we need to consider the stoichiometric ratio and the molar masses of the compounds involved in the reaction:
C₇H₆O₃ (s) + C₄H₆O₃ (s) → C₉H₈O₄ (s) + HC₂H₃O₂ (aq)
Given:
Mass of C₇H₆O₃ = 52.1 g
Assumed yield = 95.0%
First, we need to calculate the moles of C₇H₆O₃ using its molar mass:
Molar mass of C₇H₆O₃ = (7 × 12.01 g/mol) + (6 × 1.008 g/mol) + (3 × 16.00 g/mol)
= 106.12 g/mol
Moles of C₇H₆O₃ = (Mass of C₇H₆O₃) / (Molar mass of C₇H₆O₃)
= 52.1 g / 106.12 g/mol
≈ 0.491 mol
Since the reaction has a 1:1 stoichiometric ratio between C₇H₆O₃ and C₉H₈O₄, the moles of C₉H₈O₄ produced will be the same as the moles of C₇H₆O₃.
Moles of C₉H₈O₄ = 0.491 mol
To find the mass of C₉H₈O₄, we multiply the moles by its molar mass:
Molar mass of C₉H₈O₄ = (9 × 12.01 g/mol) + (8 × 1.008 g/mol) + (4 × 16.00 g/mol)
= 180.16 g/mol
Mass of C₉H₈O₄ = (Moles of C₉H₈O₄) × (Molar mass of C₉H₈O₄)
= 0.491 mol × 180.16 g/mol
≈ 88.52 g
However, we need to consider the 95.0% yield: