Homework Help is Here – Start Your Trial Now!
Science
Chemistry
How many grams of potassium chloride are produced by decomposing 118 grams of potassium chlorate ?

How many grams of potassium chloride are produced by decomposing 118 grams of potassium chlorate ?

Chemistry
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...
See similar textbooks
icon
Related questions
Question
8. How many grams of potassium chloride are produced by decomposing 118 grams of potassium chlorate ?
Name Date Period Stoichiometry Practice Problems-1 Directions: On another sheet of paper, complete the following problems. Show ALL work the CORRECT way, circle final answer, be neat, and remember sig. figs. 1. How many moles of oxygen would be required to react with calcium to produce 8 moles of calcium oxide? 2. Şodium Carbonate reacts with nitric acid to produce sodium nitrate, carbon dioxide, and water. How many moles of Sodium carbonate are required to produce 100.0 grams of sodium nitrate? 3. By using the same equation in #0, if 7.50 grams of sodium carbonate reacts, how many moles of carbon dioxide are produced? CO 2 4. Methane gas, CH4, burns in air to produce carbon dioxide and water. What mass of water is produced by burning 500. grams of methane? 5. Hydrogen peroxide breaks down releasing oxygen gas and water. What mass of oxygen is produced when 1.840 moles of hydrogen peroxide decompose? 6. By using the same equation in #4, what mass of water is produced when 5.0 moles of oxygen is produced by this reaction? 7. Chlorine gas, water, and Manganese (II) chloride can be produced in the lab by adding concentrated hydrochloric acid to Manganese (IV) oxide. Calculate the mass of Manganese (IV) oxide needed to produce 25.0 grams of chlorine gas. 8. How many grams of potassium chloride are produced by decomposing 118 grams of potassium chlorate? 9. How many moles of potassium metal would be needed to react with Fluorine gas to make 800 grams of potassium fluoride. 10. Magnesium burns in air to produce magnesium oxide. What mass of magnesium will burn in the presence of 189 mL of oxygen? The density of oxygen is 1.429 g/L.
Transcribed Image Text:Name Date Period Stoichiometry Practice Problems-1 Directions: On another sheet of paper, complete the following problems. Show ALL work the CORRECT way, circle final answer, be neat, and remember sig. figs. 1. How many moles of oxygen would be required to react with calcium to produce 8 moles of calcium oxide? 2. Şodium Carbonate reacts with nitric acid to produce sodium nitrate, carbon dioxide, and water. How many moles of Sodium carbonate are required to produce 100.0 grams of sodium nitrate? 3. By using the same equation in #0, if 7.50 grams of sodium carbonate reacts, how many moles of carbon dioxide are produced? CO 2 4. Methane gas, CH4, burns in air to produce carbon dioxide and water. What mass of water is produced by burning 500. grams of methane? 5. Hydrogen peroxide breaks down releasing oxygen gas and water. What mass of oxygen is produced when 1.840 moles of hydrogen peroxide decompose? 6. By using the same equation in #4, what mass of water is produced when 5.0 moles of oxygen is produced by this reaction? 7. Chlorine gas, water, and Manganese (II) chloride can be produced in the lab by adding concentrated hydrochloric acid to Manganese (IV) oxide. Calculate the mass of Manganese (IV) oxide needed to produce 25.0 grams of chlorine gas. 8. How many grams of potassium chloride are produced by decomposing 118 grams of potassium chlorate? 9. How many moles of potassium metal would be needed to react with Fluorine gas to make 800 grams of potassium fluoride. 10. Magnesium burns in air to produce magnesium oxide. What mass of magnesium will burn in the presence of 189 mL of oxygen? The density of oxygen is 1.429 g/L.
Expert Solution
steps

Step by step

Solved in 2 steps with 1 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Group 1 Elements
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.
Similar questions
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
SEE MORE TEXTBOOKS