A chemist finds that 30.82 g of nitrogen will react with 17.60, 35.20, 70.40, or 88.00 g of oxygen to form four different compounds. (a) Calculate the mass of oxygen per gram of nitrogen in each compound. 30.82 g N and 88.00 g O

Verified step by step guidance

Determine the mass of oxygen that reacts with one gram of nitrogen by using the ratio: Mass of Oxygen (g) / Mass of Nitrogen (g).

For the first compound, use the given masses: 17.60 g of oxygen and 30.82 g of nitrogen. Apply the ratio from step 1.

Repeat the calculation for the second compound using 35.20 g of oxygen and 30.82 g of nitrogen.

For the third compound, use 70.40 g of oxygen and 30.82 g of nitrogen and apply the ratio.

Finally, calculate for the fourth compound using 88.00 g of oxygen and 30.82 g of nitrogen.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows chemists to calculate the amounts of substances consumed and produced in a reaction based on balanced chemical equations. Understanding stoichiometry is essential for determining how much oxygen reacts with a given mass of nitrogen in this scenario.

Mass Ratio

The mass ratio is a comparison of the mass of one substance to the mass of another substance in a chemical reaction. In this case, it refers to the mass of oxygen per gram of nitrogen. Calculating this ratio helps in understanding the proportions in which elements combine to form compounds, which is crucial for analyzing the different compounds formed from nitrogen and oxygen.

Chemical Compounds

Chemical compounds are substances formed when two or more elements chemically bond together in fixed proportions. The compounds formed from nitrogen and oxygen in this question illustrate how different ratios of these elements can lead to the creation of distinct substances, such as nitrogen oxides. Recognizing the nature of these compounds is important for interpreting the results of the mass calculations.

Recommended video:

Guided course

03:37

Chemical Properties

Related Practice

Textbook Question

A 1.0-g sample of carbon dioxide (CO2) is fully decomposed into its elements, yielding 0.273 g of carbon and 0.727 g of oxygen. If a sample of a different compound decomposes into 0.429 g of carbon and 0.571 g of oxygen, what is its ratio of the mass of O to C? (c) According to Dalton's atomic theory, what is the empirical formula of the second compound?

Textbook Question

Hydrogen sulfide is composed of two elements: hydrogen and sulfur. In an experiment, 6.500 g of hydrogen sulfide is fully decomposed into its elements. b. What fundamental law does this experiment demonstrate?

Textbook Question

A chemist finds that 30.82 g of nitrogen will react with 17.60, 35.20, 70.40, or 88.00 g of oxygen to form four different compounds. (a) Calculate the mass of oxygen per gram of nitrogen in each compound. 30.82 g N and 17.60 g O

Textbook Question

A chemist finds that 30.82 g of nitrogen will react with 17.60, 35.20, 70.40, or 88.00 g of oxygen to form four different compounds. (b) How do the numbers in part (a) support Dalton's atomic theory?