Question
Given the thermochemical equation:
2 Al(s) + 3/2 O2(g) > Al2O3(s) ΔH = -95.7 kJ
find the heat of reaction, ΔH, for the following reaction:
2 Al2O3(s)> 4 Al(s) + 3 O2(g)
Select one:
a. -95.7 kJ
b. +95.7 kJ
c. -47.8 kJ
d. +47.8 kJ
e. +191.4 kJ
2 Al(s) + 3/2 O2(g) > Al2O3(s) ΔH = -95.7 kJ
find the heat of reaction, ΔH, for the following reaction:
2 Al2O3(s)> 4 Al(s) + 3 O2(g)
Select one:
a. -95.7 kJ
b. +95.7 kJ
c. -47.8 kJ
d. +47.8 kJ
e. +191.4 kJ
Answers
You have the reaction as shown. You want the reverse reaction and double that. So take dH that you have, change the sign (because of the reversal) and double it.
would it be a positive or a negative though?
it would be e...
yes.
You reversed the sign because the reaction is reversed. So that makes it positive. Then double that for e.
You reversed the sign because the reaction is reversed. So that makes it positive. Then double that for e.
thank you !!!
Related Questions
If the reaction of 2.5 g of Al with 2.5 g of O2 produced 3.5 g of Al2O3, what is the percent yield o...
According to the following thermochemical reaction, how much energy is involved in the reaction of 1...
Find the mass of AlCl3 that is produced when 10.0 grams of Al2O3 react with 25.0 g of HCl according...
Given ∆Hºrxn = -1670 kJ/mol for 2Al(s) + (3/2)O2(g) --> Al2O3(s), determine ∆Hº for the reaction 2Al...