Question

For each of the reactions, calculate the mass (in grams) of the product formed when 15.54 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant.2K(s)+Cl₂(g)→2KCl(s) (Cl₂ is underlined)

a. 31.08 g
b. 62.16 g
c. 93.24 g
d. 124.32 g

Answer 1

To calculate the mass of the product formed when 15.54 g of Cl₂ completely reacts in the equation 2K(s)+Cl₂(g)→2KCl(s), use stoichiometry. The correct answer is 62.16 g (option b).

Step-by-step explanation:

To calculate the mass of the product formed when 15.54 g of Cl₂ completely reacts in the equation 2K(s)+Cl₂(g)→2KCl(s), we need to use stoichiometry. The balanced equation tells us that 2 moles of KCl are formed for every mole of Cl₂. First, we convert the given mass of Cl₂ to moles using its molar mass (70.90 g/mol). Then, we use the mole ratio from the balanced equation to convert moles of Cl₂ to moles of KCl. Finally, we convert moles of KCl to grams using the molar mass of KCl (74.55 g/mol). The correct answer is 62.16 g (option b).