Log in
Chemistry
1
answer
0
watching
1,479
views

1) Hydrates contain water in a stoichiometric quantity. Whatdoes this mean?

2) Why can you use calcium chloride to reduce the moisture in ahumid basement area?

3) Plaster of Paris is calcium sulfate monohydrate,(CaSO4)2.H2O. (A) How many total atoms of all kinds are present?(B) On heating the hydrate, how many moles of water should bedriven off per mole of hydrate? (C) Calculate the percent of waterin the hydrate. SHOW YOUR WORK. (D) If you heat 20.00g of hydrateand drive off the water, what is the mass of the anhydrous saltremaining? SHOW YOUR WORK.

Watch
1
answer
0
watching
1,479
views

For unlimited access to Homework Help, a Homework+ subscription is required.

Avatar image
Liked by kloiebright
Nestor Rutherford
Nestor RutherfordLv2
28 Sep 2019

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions

Plaster of paris is calcium sulfate monohydrate, (CaSO4)2.H2O. If you heat 20.00g of hydrate and drive off the water, what is the mass of the anhydrous salt remaining? Show your work.

Anhydrate = MgSO4(s)

Mass of container = 21.400g

Mass of container and content before heating = 26.65g

Mass of hydrate = 5.250

Mass of container and content after heating = 23.960g

Mass of anhydrate = 2.56g

Mass of water lost = 2.69g

Calculate moles of anhydrate in sample 2.56g anhydrate*1mole anhydrate/120.3626 molar mass= 0.0213 moles of anhydrate.

Calculate the ratio of moles of water for 1 mole of anhydrate: 0.149 calculated moles of H2O/0.0213 calculated moles of anyhydrate = 6.995305164/1mole anhydrate = 7 moles H2O/1 mole MgSO4

Use the whole number values calculated in above problem to write the formula for the hydrate =MgSO4(s0*7H2O (g)

Write and equation for the dehydration of the hydrate= MgSO4(s)*7H2O(g) MgSO4 (s) + 7H2O(g)

Write an equation for the dehydration of the following hydrates;

CaCl2*2H2O CaCl2*2H2O CaCl2 +2H2O

CoCl2*6H2O CoCl2*6H2O CoCl2 + 6H2O

Na2CO3*10H2O Na2CO3H2O Na2CO3H2O + 9H2O

Calculate the % water for the hydrate, Na2CO3*10H2O

10 *18/ 286 *100% =63% H2O in Na2CO3*10H2O

If you did not heat the hydrate sample sufficiently to drive off all of the water, would the % of water calculated be too high or too low? Explain.

Aluminum and oxygen gas react to produce aluminum oxide. What is the % of oxygen in the product aluminum oxide?

Answer = 89%

Write a balanced equation for the reaction = 4Al + 6O2 2Al2O3

If 75g of oxygen react, how many grams of Aluminum are required?

How many grams of aluminum oxide can be produced form 75g of oxygen?

Can you please look over my Calculations and if they are wrong will you please explain and show how to do them. Also could you help me with the calculations that I didn’t answer.
Thanks!

Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in