Question

1.
Refer to this equation:

2CaCO3 (s) —> 2CaO (s) + 2CO2 (g)

Enthalpy change = -178.1 kJ/ mol reaction

How many grams of CaCo3 must react in order to liberate 545 kJ
of heat?

2. Refer to this equation:

2Al (s) + Fe2O3 (s) —> 2Fe (s) + Al2O3 (s)

Enthalpy change = -847.6 kJ/ mol reaction

How much heat is released if 35.0 g of Al (s) reacts to
completion?

Answer #1

1)

from reaction,

2 moles of CaCO3 liberates 178.1 KJ

So,

to liberate 545 KJ, moles of CaCO3 required = 2*(545/178.1)

= 6.12 mol

Molar mass of CaCO3 = 1*MM(Ca) + 1*MM(C) + 3*MM(O)

= 1*40.08 + 1*12.01 + 3*16.0

= 100.09 g/mol

we have below equation to be used:

mass of CaCO3,

m = number of mol * molar mass

= 6.12 mol * 100.09 g/mol

= 613 g

Answer: 613 g

Only 1 question at a time please

Given that: 2Al(s) + 3/2O2(g) -->
Al2O3(s) Delta H degrees rxn =-1601kJ/mol
and 2Fe(s) + 3/2O2(g) -->
Fe2O3(s) Delta H degrees rxn =-821kJ/mol
Calculate the standard enthalpy change for the following
reaction: 2Al(s) + Fe2O3(s) --> 2Fe(s) +
Al2O3(s)
Answer in scientific notation

Calculate the standard enthalpy change for the reaction
2 Al(s) +
Fe2O3(s)
2
Fe(s) + Al2O3(s)
Given that
2 Al(s) + 3/2 O2
(g)
Al2O3(s) ΔH rxn =
-1669.8 kJ/mol
2 Fe (s) +
3/2 O2
(g)
Fe2O3(s) ΔH rxn = -822.2
kJ/mol

A chemist measures the enthalpy change ΔH during the following
reaction: 2Al (s) + Fe2O3 (s) → Al2O3 (s) + 2Fe (s) =ΔH−852.kJ
Use this information to calculate ΔH in kJ for the following
reactions:
3Al2O3s + 6Fes → 6Als +
3Fe2O3s
Al2O3s + 2Fes → 2Als +
Fe2O3s
4Als + 2Fe2O3s → 2Al2O3s +
4Fes

Calculate the enthalpy of reaction for the following reaction:
Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ΔHfo(Fe2O3(s)) = -824.2 kJ/mol
ΔHfo(CO(g)) = -110.5 ΔHfo(Fe(s)) = ? ΔHfo(CO2(g)) = -393.5
kJ/mol

C2N2O2Hg(s) + O2 (g)
-> Hg(g) + 2CO2(g) + N2(g)
Determine the theoretical enthalpy (in kJ/mol) of the mercury
fulminate reaction by using the enthalpy of formation for mercury
fulminate (+ 386 kJ/mol) Remember, ΔH° rxn = Σn x
H°f(products) - Σn x ΔH°f(reactants). Explain
your work. We are assuming a constant pressure situation.
This is can also be termed the heat of
explosion, but when it is termed heat of explosion,
the units are traditionally kJ/kg of substance. Convert...

Given the following reactions:
Question (1)
Calculate for the change in enthalpy of the reaction of
(3Fe2O3(s) + CO(g) yields CO2(g) + 2Fe3O4(s))
Fe2O3(s) + 3CO(g) yields 2Fe(s) + 3CO2(s)(Change in enthalpy=
-28.0 kJ)
3Fe(s) + 4CO2(s) yields 4CO(g) + FE3O4(s) (Change in enthalpy=
+12.5 kJ)

What is the enthalpy change for the first reaction?
P4(s) + 6Cl2(g) → 4PCl3(l) ΔH
=
P4(s) + 10Cl2(g) → 4PCl5(s) ΔH
= -1,779.8
PCl3(l) + Cl2 → PCl5(s) ΔH =
-123.3
question 2
What is the enthalpy change for the first reaction?
Fe2O3(s) → 2Fe(s) + 3/2O2(g) ΔH
=
4Fe(s) + 3O2(g) → 2Fe2O3 (s) ΔH
= -1,645 kJ
Help me understand, please

What is the maximum theoretical number of moles of aluminum
oxide that can be recovered from the reaction of 27.7 mol of
aluminum and 27.8 moles of oxygen gas?
4 Al (s) + 3 O2(g) → 2
Al2O3(s)
What mass of aluminum oxide can be recovered from the complete
reaction of 34.3 g of Al with 34.3 g of oxygen gas?
4 Al (s) + 3 O2(g) → 2
Al2O3(s)
If 8.7 moles of Al and 3.2 moles of Fe2O3...

1)
Calculate the change in enthalpy (in kJ) for the reaction using
the Enthalpy tables in
the back of your book.
CaCO3(s) CaO(s) + CO2(g)
2)
5. The combustion of ethane, C2H4, is an exothermic
reaction.
C2H4(g) + 3 O2(g) 2 CO2(g) + 2 H2O(l) ∆H = -1.39 x 103
J
Calculate the amount of heat liberated when 4.79 g of C2H4 reacts
with excess oxygen.

A scientist measures the standard enthalpy change for this
reaction to be 163.2 kJ/mol. CaCO3(s)CaO(s) + CO2(g) Based on this
value and the standard formation enthalpies for the other
substances, the standard formation enthalpy of CO2(g) is ____
kJ/mol.

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