Calculate the mass (in grams) of the product formed when 10.1g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant.

2K(s) + __Cl2(g)__ -> 2KCl(s)

I cannot get the correct answer.

determine how many moles of chlrine 10.1 grams represents.

That number, times two, is the number of moles of KCl. Change that amount of moles to grams of KCl.

To calculate the mass of the product formed, we need to determine the molar mass of the reactant that completely reacts and use it to find the molar mass of the product.

In this equation, the reactant that is underlined is Cl2. The molar mass of Cl2 can be found by adding up the molar masses of two chlorine atoms (Cl).

The molar mass of Cl is approximately 35.45 g/mol. Therefore, the molar mass of Cl2 is:
Molar mass of Cl2 = 2 x Molar mass of Cl = 2 x 35.45 g/mol = 70.90 g/mol

Since we know the mass of Cl2 (10.1 g), we can use the molar mass of Cl2 to find the number of moles of Cl2:
Number of moles = Mass / Molar mass
Number of moles of Cl2 = 10.1 g / 70.90 g/mol ≈ 0.142 mol (rounded to 3 decimal places)

Now, according to the balanced equation, 2 moles of KCl are produced for every 1 mole of Cl2 reacted. Therefore, the number of moles of KCl produced will also be 0.142 mol.

Finally, to find the mass of KCl produced, we multiply the number of moles by the molar mass of KCl:
Mass of KCl = Number of moles x Molar mass
Mass of KCl = 0.142 mol x (2 x Molar mass of K + Molar mass of Cl)
Mass of KCl = 0.142 mol x (2 x 39.10 g/mol + 35.45 g/mol) ≈ 11.11 g (rounded to 2 decimal places)

Therefore, the mass of the product formed when 10.1 g of Cl2 completely reacts is approximately 11.11 grams.