Log in
Chemistry
2
answers
0
watching
132
views

1. Magnesium metal reacts with HCl to produce MgCl­2 (aq) and hydrogen gas. When 1.50 grams of magnesium metal is allowed to react with 200 mL of 6.00 M aqueous HCl, the temperature rises from 25.0 C to 42.9C. Calculate H for the reaction assuming that the specific heat of the final solution is 4.184 J/gC and the density of the solution is 1.00g/mL.

Watch
2
answers
0
watching
132
views

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

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
Share
Bunny Greenfelder
Bunny GreenfelderLv2
28 Sep 2019
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

when 1.50 g of magnesium metal is allowed to react with 200 mLof 6.00 M aqueous HCl, the temperature rises from 25.0 celsuis to42.9 celsius. calculate deltaH in kilojoules for the reaction,assuming that the heat capacity of the calorimeter is 776j/celsius, that the specific heat of the final solution is the sameas that of water(4.184J/G*C), and that the density of the solutionis 1.00 g/ml.

When 1.50g of magnesium metal is allowed to react with 200mL of6.00M aqueous HCl, the temperature rises from 25.0 degrees Celsiusto 42.9 degrees Celsius. Calculate delta H (in kilojoules) for thereaction, assuming that the heat capacity of the calorimeter is 776Joules/degrees celsius, that the specific heat of the finalsolution is the same as that of water (4.18J/g degrees celsius),and that the density of the solution is 1.00 g/mL.

I'm stuck because I'm not sure what equation for delta H to use.I thought it would be equal to q, but I'm not sure how to go aboutthat either.

An unknown metal weighing 13.11g at a temperature of 81.0C is placed in a calorimeter containing 25.0 mL of water at a temp of 25.0 C. The final equilibrium temp is 30.0 C. What is the specific heat of the metal? The specific heat of water is 4.184 J/gxC. Assume the density of th water is 1.00g/mL and there is no heat lost or gained by the calorimeter.

Please show work

Weekly leaderboard

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