Given: 2C₆H₅COOH + Na₂CO₃ $\rightarrow$2C₆H₅COONa + H₂O + CO₂ What mass of CO₂ is formed when 275 mL of 0.150 M Na₂CO₃is mixed with 775 mL of 0.254 M C₆H₅COOH? A) 2.54 g B) 3.63 g C) 1.82 g D) 6.36 g E) 4.52 g

Question

Quizplus · Accepted Answer

First, balance the equation: 2NaCO₂ + 3C₆H₅COOH → CO₂ + Na2₂O3 + 3H2₂COONa Next, use the given volumes and concentrations to calculate the moles of each reactant: moles Na₂CO₃ = (0.150 mol/L)(0.275 L) = 0.0413 mol moles C₆H₅COOH = (0.254 mol/L)(0.775 L) = 0.197 mol Using stoichiometry, we can see that the reaction produces 1 mole of CO₂ for every 2 moles of Na₂CO₃ consumed: 0.0413 mol Na₂CO₃ × (1 mol CO₂ / 2 mol Na₂CO₃) = 0.0207 mol CO₂ Finally, use the molar mass of CO₂ to convert from moles to grams: 0.0207 mol CO₂ × (12.01 g/mol + 32.07 g/mol + 12.01 g/mol) = 1.82 g CO₂ Therefore, the answer is choice C (1.82 g).

Given: 2C6H5COOH + Na2CO3 →\rightarrow→ 2C6H5COONa + H2O + CO2 What Mass of CO2 Is

Given: 2C₆H₅COOH + Na₂CO₃ $\rightarrow$ 2C₆H₅COONa + H₂O + CO₂ What Mass of CO₂ Is