A sample of a salt of nickel and phosphorus contains 2.348 g of nickel metal and 0.827 g of phosphorus. Determine the empirical formula of the salt. aldio vns to eM

Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
icon
Related questions
Question
100%
What is the empirical formula
**Problem 1: Determining the Empirical Formula**

A sample of a salt composed of nickel and phosphorus contains 2.348 grams of nickel metal and 0.827 grams of phosphorus. Determine the empirical formula of the salt.

**Solution Steps:**

1. **Convert Mass to Moles:**
   - Calculate the moles of nickel (Ni) by dividing by its molar mass.
   - Calculate the moles of phosphorus (P) by dividing by its molar mass.

2. **Determine the Mole Ratio:**
   - Divide the moles of each element by the smallest number of moles obtained in the previous step.

3. **Write the Empirical Formula:**
   - Use the mole ratio to assign subscripts to each element in the chemical formula.

This problem involves understanding the concept of empirical formulas and how to derive them from given masses of elements in a compound.
Transcribed Image Text:**Problem 1: Determining the Empirical Formula** A sample of a salt composed of nickel and phosphorus contains 2.348 grams of nickel metal and 0.827 grams of phosphorus. Determine the empirical formula of the salt. **Solution Steps:** 1. **Convert Mass to Moles:** - Calculate the moles of nickel (Ni) by dividing by its molar mass. - Calculate the moles of phosphorus (P) by dividing by its molar mass. 2. **Determine the Mole Ratio:** - Divide the moles of each element by the smallest number of moles obtained in the previous step. 3. **Write the Empirical Formula:** - Use the mole ratio to assign subscripts to each element in the chemical formula. This problem involves understanding the concept of empirical formulas and how to derive them from given masses of elements in a compound.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 4 steps

Blurred answer
Knowledge Booster
Mole Concept
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY