Question

For the reaction 2Sr(s)+O₂(g)→2SrO(s) calculate how many grams of the product form when 21.4 g of Sr completely reacts. Assume that there is more than enough of the other reactant.

Answer 1

To calculate the grams of SrO produced, we use stoichiometry. First, calculate the moles of Sr using its molar mass. Then, use the balanced equation to find the mole ratio between Sr and SrO. Finally, convert the moles of SrO to grams using the molar mass of SrO.

Step-by-step explanation:

To calculate the grams of the product formed in the given reaction, we need to use stoichiometry. First, we determine the number of moles of Sr using its molar mass. Then, we use the balanced chemical equation to find the mole ratio between Sr and SrO. Finally, we convert the moles of SrO to grams using the molar mass of SrO.

Given that the molar mass of Sr is 87.62 g/mol and the molar mass of SrO is 103.62 g/mol, we calculate:

Moles of Sr = 21.4 g / 87.62 g/mol = 0.244 mol Sr

Moles of SrO = 0.244 mol Sr x (2 mol SrO / 2 mol Sr) = 0.244 mol SrO

Grams of SrO = 0.244 mol SrO x 103.62 g/mol = 25.3 g SrO