Question

42. The standard enthalpies of formation of NO (g), NO2 (g), and N2O3 (g) are 90.25...

42. The standard enthalpies of formation of NO (g), NO2 (g), and N2O3 (g) are 90.25 kJ mole-1, 33.2 kJ mole-1, and 83.72 kJ mole-1, respectively. Their standard entropies are 210.65 J mole-1 K-1, 239.9 J mole-1 K-1, and 312.2 J mole-1 K-1 respectively.

(a) Use the data above to calculate the free energy change for the following reaction at 25.0 o C.
N2O3 (g) -------> NO (g) + NO2 (g)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)→NO2(g),   ΔH∘A=33.2...
Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)→NO2(g),   ΔH∘A=33.2 kJ 12N2(g)+12O2(g)→NO(g),  ΔH∘B=90.2 kJ
The values for the standard formation enthalpies at 298.15K for CO (g), and H2O(g) are -...
The values for the standard formation enthalpies at 298.15K for CO (g), and H2O(g) are - 110.53 kJ/mol and - 241.82 kJ/mol, respectively. The molar heat capacities of products and reactants are given as: CPm Ø (H2(g)) = 28.824 J/K.mol, CPm Ø (CO(g)) = 29.140 J/mol.K, CPm Ø (H2O(g)) = 33.580 J/mol.K, CPm Ø (C(s, graphite)) = 8.527 J/mol.K Calculate Delta (reaction) U in kJ for the formation at 378.15 K and 1 bar of 6.54 g CO(g) following the...
Using the table of standard entropies and enthalpies of formation, calculate ΔH°, ΔS°, and ΔG° for...
Using the table of standard entropies and enthalpies of formation, calculate ΔH°, ΔS°, and ΔG° for the following reactions at 298.15 K. (Use only the table of standard entropies and standard enthalpies of formation, not the table of standard Gibbs free energies.) Compound ΔHof (kJmol)ΔHfo (kJmol) ΔSof (Jmol⋅K)ΔSfo (Jmol⋅K) The equation SiO2(s) + 2 Mg(s) → Si(s) + 2 MgO(s) ΔHoΔHo  kJ ΔSoΔSo  J/K ΔGoΔGo  kJ C(s) 0 5.7 CO(g) -110.5 197.7 CO2(g) -393.5 213.8 Cl2(g) 0 223.1 H2(g) 0 130.7 HCl(g) -92.3...
Thermodynamics: Consider the equilibrium reaction A(g) + B(g) -><- C(g)+D(g). At T=298 K, the standard enthalpies...
Thermodynamics: Consider the equilibrium reaction A(g) + B(g) -><- C(g)+D(g). At T=298 K, the standard enthalpies of formation of the components in the gas phase are -20, -40, -30, and -10 kJ/mol for A,B,C, and D, respectively. The standard-state entropies of the components in the gas phase are 30, 50, 50, and 80 J/(mol K), in the same order. The vapor pressure of liquid C at this temperature is 0.1 bar, while all other components are volatile gases with Henry's...
Standard enthalpies of fromation are usually computed from the calorimetric data referring to reactions, which are...
Standard enthalpies of fromation are usually computed from the calorimetric data referring to reactions, which are easy to carry out in the laboratory. For many compounds, the enthalpy of the reaction with O2 (g) (combustion) is commonly used, together with the standard enthalpies of formation of the combustion products, to compute ΔHf°. For example, sucrose C12H22O11, common table sugar, is found to have a standard enthalpy of combustion of -5640.9 kJ/mole. The standard enthalpies of formation of CO2 (g) and...
-4 Question 1: The standard formation enthalpies at 25.00 ° C for methanol (CH4O (1)), water...
-4 Question 1: The standard formation enthalpies at 25.00 ° C for methanol (CH4O (1)), water (H2O (1)) and carbon dioxide (CO2 (g)) are respectively -238.7 kJ mol, 285.8 kJ / mol, and -393.5 kJ / mol. Calculates the change in the environment (in J / K) when burning 13.5 g of methanol under a constant pressure of 1,000 atm at 25.00 oC (NB, combustion is the reaction of a substance with oxygen) Molecular to produce water and carbon dioxide)....
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of...
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) NO(g) 90.2 O2(g) 0 NO2(g) 33.2 Then the standard heat...
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of...
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g) with heat of formation values given by the following table: Substance   ΔH∘f (kJ/mol) NO(g)   90.2 O2(g)   0 NO2(g)   33.2 Then the standard heat...
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of...
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) NO(g) 90.2 O2(g) 0 NO2(g) 33.2 Then the standard heat...
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...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT