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?
Ch.2 - Atoms, Molecules, and Ions
Chapter 2, Problem 13a2
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 35.20 g O
Verified step by step guidance1
Identify the given masses of nitrogen and oxygen: 30.82 g of nitrogen and 35.20 g of oxygen.
Understand that you need to find the mass of oxygen per gram of nitrogen for the given compound.
Set up the ratio of the mass of oxygen to the mass of nitrogen: \( \frac{\text{mass of oxygen}}{\text{mass of nitrogen}} = \frac{35.20 \text{ g}}{30.82 \text{ g}} \).
Simplify the ratio to find the mass of oxygen per gram of nitrogen.
Express the simplified ratio as the mass of oxygen per 1 gram 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:
1mWas 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.
Recommended video:
Guided course
01:16
Stoichiometry Concept
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, calculating the mass of oxygen per gram of nitrogen involves finding the ratio of the mass of oxygen to the mass of nitrogen. This concept is crucial for understanding how different compounds can form from varying amounts of reactants.
Recommended video:
Guided course
02:14Neutron-Proton Ratio
Chemical Compounds
Chemical compounds are substances formed when two or more elements chemically bond together in fixed proportions. The different masses of oxygen reacting with a constant mass of nitrogen indicate the formation of different compounds, which can have distinct properties. Recognizing how these compounds differ based on their elemental composition is key to interpreting the results of the reaction.
Recommended video:
Guided course
03:37Chemical Properties
Related Practice
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. (a) Calculate the mass of oxygen per gram of nitrogen in each compound. 30.82 g N and 88.00 g O
1
rank
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 70.40 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?
Textbook Question
In a series of experiments, a chemist prepared three different compounds that contain only iodine and fluorine and determined the mass of each element in each compound: Compound Mass of Iodine (g) Mass of Fluorine (g) 1 4.75 3.56 2 7.64 3.43 3 9.41 9.86 (a) Calculate the mass of fluorine per gram of iodine in Compound 3.