Question
The enthalpy of formation of AB2(l) from A2(g) and B2(g) at 545.5*K is -642.4 kJ/mol. Determine...
The enthalpy of formation of AB2(l) from A2(g) and B2(g) at 545.5*K is -642.4 kJ/mol. Determine (delta)E for this process at 543.5*K (4 significant figures)
Homework Answers
Answer #1
A2(g) + 2 B2 (g) ---------------------> 2 AB2 (l) , 
H =
-642.4 kJ / mol
n = products -
reactants
= 0 -(1 + 2 )
= -3
H = E +
n RT
-642.4 = E - 3 x 8.314 x
10^-3 x 545.5
E = -628.8 kJ /
mol
Not the answer you're looking for?
Similar Questions
Standard enthalpies of formation are obtained from thermodynamic tables as: C2H5OH(l) -224 kJ/mol CO2(g) -398 kJ/mol...
Standard enthalpies of formation are obtained from
thermodynamic tables as:
C2H5OH(l) -224 kJ/mol
CO2(g) -398 kJ/mol
H2O(l) -281 kJ/mol.
Calculate the enthalpy change of the reaction
C2H5OH(l) + 3 O2 ? 2 CO2(g) + 3 H2O
Follow the procedures based on Hess's Law:
First write down the reactions corresponding to the enthalpies
of formation you have been given, reverse the equations if
necessary, remembering to change the sign of ?Ho, then combine the
equations to give the required process, and...
The enthalpy of vapourization of benzene(l) to benzene(g) is +33.0 kJ/mol. a)From the BE values in...
The enthalpy of vapourization of benzene(l) to benzene(g) is
+33.0 kJ/mol.
a)From the BE values in Table 3.1, and again the enthalpy of
atomization of C(s), +717 kJ/mol, estimate the enthalpy of
formation of benzene(l). (Hint: now the formation of benzene(g) has
to be followed by the reaction benzene(g)®benzene(l), the opposite
of vapourization).
The standard molar enthalpy of formation for gaseous H2O is −241.8 kJ/mol. What is the standard...
The standard molar enthalpy of formation for gaseous H2O is
−241.8 kJ/mol. What is the standard molar enthalpy of formation for
liquid hydrazine (N2H4)?
N2H4(l) + O2(g) → N2(g) + 2H2O(g)
ΔH° = ‒534.2 kJ
‒292 kJ/mol
292 kJ/mol
‒146 kJ/mol
50.6 kJ/mol
‒50.6 kJ/mol
Calculate the standard enthalpy of formation of Ga2H6(g) (in kJ/mol) from the following data: 2 Ga(s)...
Calculate the standard enthalpy of formation of Ga2H6(g) (in
kJ/mol) from the following data:
2 Ga(s) + 3/2 O2(g)-->Ga2O3(s). ΔHo = –1188
kJ/mol
Ga2H6(g) + 3 O2(g)-->Ga2O3(s) + 3 H2O(l). ΔHo = –2158 kJ/mol
H2(g) + 1/2 O2(g)--> H2O(g) ΔHo = –242 kJ/mol
H2O(l)-->H2O(g) ΔHo = +44 kJ/mol
2 Ga(s) + 3 H2(g)-->Ga2H6(g). ΔHo = ? kJ/mol
Standard enthalpies of formation are obtained from thermodynamic tables as: C2H5OH(l) -227 kJ/mol CO2(g) -390...
Standard enthalpies of formation are obtained from thermodynamic
tables as:
C2H5OH(l) -227 kJ/mol
CO2(g) -390 kJ/mol
H2O(l) -285 kJ/mol.
Calculate the enthalpy change of the
reaction
C2H5OH(l) + 3 O2 ? 2
CO2(g) + 3 H2O
Follow the procedures based on Hess's Law:
First write down the reactions corresponding to the enthalpies of
formation you have been given, reverse the equations if necessary,
remembering to change the sign of ?Ho, then combine the
equations to give the required...
The standard enthalpy of formation of the fumarate ion is ∆fHo = -777.4 kJ mol-1. If...
The standard enthalpy of formation
of the fumarate ion is ∆fHo = -777.4 kJ
mol-1. If the standard enthalpy change of the
reaction,
fumarate2- (aq) +
H2(g) → succinate2- (aq), is 131.4 kJ
mol-1, what is the enthalpy of formation of the
succinate ion?
Data Tables Heats of Formation Compound delta Hf (kJ mol-1) H20 (l) -285.83 CO2 (g) -391.51...
Data Tables
Heats of Formation
Compound delta Hf (kJ mol-1)
H20 (l) -285.83
CO2 (g) -391.51
Bond Enthalpies
Reaction delta H (298K)
C(s, graphite) to C(g) 716.7
H-H to 2H(g) 436
C-H to C(g) + H(g)
413 C-C to 2C(g) 348
*****For the word "to" it means arrow, or reacts to form this
(not able to put an arrow on here)
a) If the standard enthalpy of combustion of gaseous
cyclopropane, C3H6, is -2091.2kJ mol-1 at 25 C, calculate the...
1. The standard enthalpy of formation of phenol is -165.0 kJ/mol. Calculate its standard enthalpy of...
1. The standard enthalpy of formation of phenol is
-165.0 kJ/mol. Calculate its standard enthalpy of combustion.
[Express your answer in units of kilojoules per mole,
kJ/mol]
C6H5OH + 7O2 --> 6 CO2 + 3H2O
ΔHc = 6ΔHf(CO2) + 3ΔHf(H2O) - ΔHf(C6H5OH) - 7ΔHf(O2)
2. Calculate the work done on a closed system consisting
of 50.0 grams of argon, assumed ideal, when it expands isothermally
and reversibly from a volume of 5.00 L to a volume of 10.00 L at...
The standard enthalpy change for this reaction is -731 kJ/mol at 298 K. 2 N2(g) +...
The standard enthalpy change for this reaction is -731 kJ/mol at
298 K. 2 N2(g) + 4 H2(g) + 3 O2(g) = 2 NH4NO3(s) ΔrH° = -731 kJ/mol
Calculate the standard enthalpy change for the reaction N2(g) + 2
H2(g) + 3/2 O2(g) = NH4NO3(s) at 298 K.
The standard enthalpy of formation of benzoic acid, C6H5COOH, is −385kJ mol−1 at 298 K. Calculate...
The standard enthalpy of formation of benzoic acid,
C6H5COOH, is −385kJ mol−1 at 298
K. Calculate the standard enthalpy of combustion of benzoic acid at
this temperature, given that the standard enthalpy of formation of
liquid water, H2O is −285.8 kJ mol−1 and
gaseous carbon dioxide, CO2, is −393.51 kJ
mol−1.
A
−294.3 kJ mol−1
B
−3997kJ mol−1
C
−3227.0 kJ mol−1
D
2282.2 kJ mol−1
ADVERTISEMENT
Need Online Homework Help?
Get Answers For Free
Most questions answered within 1 hours.
ADVERTISEMENT
Active Questions
asked 13 minutes ago
asked 29 minutes ago
asked 29 minutes ago
asked 31 minutes ago
asked 39 minutes ago
asked 44 minutes ago
asked 48 minutes ago
asked 48 minutes ago
asked 51 minutes ago
asked 58 minutes ago
asked 1 hour ago
asked 1 hour ago