Determine the chemical formula of each compound and then use it to calculate the mass percent composition of each constituent element. c. nitrogen triiodide

Verified step by step guidance

Identify the chemical formula of nitrogen triiodide, which is \( \text{NI}_3 \).

Determine the molar mass of each element in the compound: nitrogen (N) and iodine (I).

Calculate the molar mass of nitrogen triiodide (\( \text{NI}_3 \)) by adding the molar mass of one nitrogen atom and three iodine atoms.

Calculate the mass percent composition of nitrogen by dividing the molar mass of nitrogen by the molar mass of \( \text{NI}_3 \) and multiplying by 100%.

Calculate the mass percent composition of iodine by dividing the total molar mass of iodine (3 atoms) by the molar mass of \( \text{NI}_3 \) and multiplying by 100%.

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.

Chemical Formula

A chemical formula represents the composition of a compound, indicating the types and numbers of atoms present. For nitrogen triiodide, the formula is NI3, which shows one nitrogen atom and three iodine atoms. Understanding how to derive and interpret chemical formulas is essential for analyzing compounds and their properties.

Mass Percent Composition

Mass percent composition is a way to express the relative amounts of each element in a compound as a percentage of the total mass. It is calculated by dividing the mass of each element in one mole of the compound by the molar mass of the compound, then multiplying by 100. This concept is crucial for understanding the distribution of elements within a compound.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all atoms in the chemical formula. For nitrogen triiodide, knowing the molar mass allows for accurate calculations of mass percent composition and is fundamental in stoichiometry and chemical reactions.

Recommended video:

Guided course

02:11

Molar Mass Concept

Related Practice

Textbook Question

A drop of water has a volume of approximately 0.05 mL. How many water molecules does it contain? The density of water is 1.0 g/cm³.

Textbook Question

Determine the chemical formula of each compound and then use it to calculate the mass percent composition of each constituent element. a. potassium chromate b. lead(II) phosphate

Textbook Question

Determine the chemical formula of each compound and then use it to calculate the mass percent composition of each constituent element. c. sulfurous acid

Textbook Question

A Freon leak in the air-conditioning system of an old car releases 38.0 g of CF2Cl2 per month. What mass of chlorine does this car emit into the atmosphere each year?

Textbook Question

Determine the chemical formula of each compound and then use it to calculate the mass percent composition of each constituent element. d. cobalt(II) bromide

Textbook Question

A metal (M) forms a compound with the formula MCl₃. If the compound contains 65.57% Cl by mass, what is the identity of the metal?

views