We’re being asked to find the formula of an oxide of carbon in which the ratio by mass of oxygen to carbon is 2.00:1.00.
We’re given the ratio of oxygen (O) to carbon (C) by mass in carbon monoxide is 1.33:1.00.
According to the Law of Multiple Proportions, when two elements (A & B) form different compounds, the masses of element B that combine with 1 g of A are a ratio of whole numbers.
Hydrazine, ammonia, and hydrogen azide all contain only nitrogen and hydrogen. The mass of hydrogen that combines with 1.00 g of nitrogen for each compound is 1.44x 10-1 g, 2.16 x 10-1 g, and 2.40 x 10-2 g, respectively. Show how these data illustrate the law of multiple proportions.
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Law of Multiple Proportions concept. You can view video lessons to learn Law of Multiple Proportions. Or if you need more Law of Multiple Proportions practice, you can also practice Law of Multiple Proportions practice problems.
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Based on our data, we think this problem is relevant for Professor Kelleher's class at BU.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.