Tungsten (W) reacts with Cl₂ to form WCl₆. What mass of WCl₆ is formed from the reaction of 12.6 g W with 13.6 g Cl₂?

Question

Quizplus · Accepted Answer

To solve this problem, we need to first write out the balanced chemical equation for the reaction: W + Cl₂ → WCl₆ Next, we need to determine the limiting reactant. We can do this by calculating the number of moles of each reactant: moles of W = 12.6 g / 183.84 g/mol = 0.0685 mol moles of Cl₂ = 13.6 g / 190.76 g/mol = 0.0713 mol Since W is the limiting reactant (it produces fewer moles of product than Cl₂), we will use its mole ratio with the product to calculate the mass of product formed: 1 mol W : 1 mol WCl₆ 0.0685 mol W : x mol WCl₆ x = 0.0685 mol Finally, we can convert the number of moles of product to grams: mass of WCl₆ = 0.0685 mol × 342.32 g/mol = 23.4 g Therefore, the correct answer is D) 25.4 g (the closest option to 23.4 g).

Tungsten (W) Reacts with Cl2 to Form WCl6

Tungsten (W) Reacts with Cl₂ to Form WCl₆