9. a fire in the lab is calculated to consume 17.9 moles of oxygen (o₂), how many grams of o₂ is this?
9. a fire in the lab is calculated to consume 17.9 moles of oxygen (o₂), how many grams of o₂ is this?
Answer
Explanation:
Step1: Determine the molar mass of (O_2)
The molar mass of (O) (oxygen atom) is (16\space g/mol). For (O_2), (M = 2\times16\space g/mol=32\space g/mol)
Step2: Use the formula (m = n\times M)
Given (n = 17.9\space mol) (moles of (O_2)) and (M = 32\space g/mol) (molar mass of (O_2)). Then (m=17.9\space mol\times32\space g/mol) [m = 17.9\times32= 572.8\space g]
Answer:
(572.8\space g)