IDNLearn.com: Your one-stop platform for getting reliable answers to any question. Our platform offers detailed and accurate responses from experts, helping you navigate any topic with confidence.
A compound is made of hydrogen and oxygen.
What is the percent oxygen by mass if a sample contains 2.0 g of hydrogen and 33.0 g of oxygen?
A. [tex]$94.3 \%$[/tex] B. [tex]$5.71 \%$[/tex] C. [tex]$0.0571 \%$[/tex] D. [tex]$0.943 \%$[/tex]
To determine the percent oxygen by mass in a compound that contains 2.0 grams of hydrogen and 33.0 grams of oxygen, follow these steps:
1. Calculate the total mass of the compound: - The mass of hydrogen = 2.0 grams - The mass of oxygen = 33.0 grams - Total mass = mass of hydrogen + mass of oxygen - Total mass = 2.0 g + 33.0 g = 35.0 grams
2. Calculate the percent oxygen by mass: - Percent mass of oxygen = (mass of oxygen / total mass) 100 - Percent mass of oxygen = (33.0 g / 35.0 g) 100
3. Perform the division and multiplication: - Mass ratio = 33.0 / 35.0 ≈ 0.942857 - Percent mass of oxygen = 0.942857 * 100 ≈ 94.3%
So, the percent oxygen by mass in the compound is approximately [tex]\( 94.3\% \)[/tex].
Therefore, the correct answer is: [tex]\[ 94.3 \% \][/tex]
We appreciate your participation in this forum. Keep exploring, asking questions, and sharing your insights with the community. Together, we can find the best solutions. Your search for answers ends at IDNLearn.com. Thanks for visiting, and we look forward to helping you again soon.
