Question

Calculate the standard enthalpy of formation of dinitrogen pentoxide (N2O5) using the following thermochemical information: 2...

Calculate the standard enthalpy of formation of dinitrogen pentoxide (N2O5) using the following thermochemical information: 2 H2O(l) 2 H2(g) + O2(g) H = +571.7 kJ 2 HNO3(l) N2O5(g) + H2O(l) H = +92.0 kJ N2(g) + 3 O2(g) + H2(g) 2 HNO3(l) H = -348.2 kJ H = kJ

Homework Answers

Answer #1

If you have any query please comment

If you satisfied with the solution please rate it thanks

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Calculate the standard enthalpy of formation of liquid water (H2O) using the following thermochemical information: 4...
Calculate the standard enthalpy of formation of liquid water (H2O) using the following thermochemical information: 4 B(s) + 3 O2(g) 2 B2O3(s) H = -2509.1 kJ B2H6(g) + 3 O2(g) B2O3(s) + 3 H2O(l) H = -2147.5 kJ B2H6(g) 2 B(s) + 3 H2(g) H = -35.4 kJ
1.) Using enthalpies of formation, calculate the standard change in enthalpy for the thermite reaction. The...
1.) Using enthalpies of formation, calculate the standard change in enthalpy for the thermite reaction. The enthalpy of formation of Fe3O4 is −1117 kJ/mol. 8 Al(s) + 3 Fe3O4(s) → 4 Al2O3(s) + 9 Fe(s) 2. a) Nitroglycerin is a powerful explosive, giving four different gases when detonated. 2 C3H5(NO3)3(l) → 3 N2(g) + 1/2 O2 (g) + 6 CO2(g) + 5 H2O(g) Given that the enthalpy of formation of nitroglycerin, ΔHf°, is −364 kJ/mol, calculate the energy (heat at...
Using the information below determine the change in enthalpy for the following reaction:             2NO(g) +...
Using the information below determine the change in enthalpy for the following reaction:             2NO(g) + 5 H2(g) → 2NH3(g) + 2H2O(l) H2(g) + ½ O2(g) →   H2O(l)                     ∆H°= -285.8kJ N2(g) + O2(g)   → 2NO(g)                     ∆H°= +180.5 kJ 2NH3(g) → N2(g) + 3H2(g)                    ∆H°= + 92.22 kJ please explain step by step! thanks!
9. Use the following experimentally derived combustion data to calculate the standard molar enthalpy of formation...
9. Use the following experimentally derived combustion data to calculate the standard molar enthalpy of formation (ΔH°f ) of liquid methanol (CH3OH) from its elements. 2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(l)     ΔH°rxn = −1452.8 kJ C(graphite) + O2(g) → CO2(g)                               ΔH°rxn = −393.5 kJ 2 H2(g) + O2(g) → 2 H2O(l)                                     ΔH°rxn = −571.6 kJ (1) −238.7 kJ/mol    (2) 487.7 kJ/mol       (3) −548.3 kJ/mol    (4) 20.1 kJ/mol         (5) 47.1 kJ/mol
Given the following information below, use Hess’s Law to calculate the enthalpy of formation for sodium...
Given the following information below, use Hess’s Law to calculate the enthalpy of formation for sodium oxide: Na (s)     +      HCl (l)  à    NaCl (aq) + ½ H2 (g)                ∆HRx = -393.1 kJ/mol Na2O (s)     +     2 HCl (l)  à 2 NaCl (aq)   + H2O              ∆HRx = -675.2 kJ/mol H2 (g)       +      ½ O2 (g)  à    H2O (g)                              ∆HRx = -288.1 kJ/mol 2 Na (s)       +       ½ O2 (g)   à   Na2O (s)                          ∆HRx =    __________ kJ/mol Calculated Heat of Reaction is....? (Put your answer in...
Calculate the heat of reaction, ∆H°, for the following reaction using Standard Enthalpy of Formation 3...
Calculate the heat of reaction, ∆H°, for the following reaction using Standard Enthalpy of Formation 3 FeCl2(s) + 4 H2O(g) --> Fe3O4(s) + 6 HCl(g) + H2(g)
Use tabulated standard molar enthalpy changes of formation to calculate Delta H rxn for the following...
Use tabulated standard molar enthalpy changes of formation to calculate Delta H rxn for the following (unbalanced) reactions: SHOW WORK a. N2O4 (g) + H2 (g) --> N2 (g) + H2O(g) b. H2S (g) + O2 (g) --> SO2 (g) + H2O(g) c. Fe2O3 (s) + HCl(g) --> FeCl3 (s) + H2O(g)
Dinitrogen pentoxide (N2O5) decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition...
Dinitrogen pentoxide (N2O5) decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition is first order with a rate constant at 45 ∘C of 1.0×10−5s−1. Part A Calculate the partial pressure of O2 produced from 1.44 L of 0.543 M N2O5 solution at 45 ∘C over a period of 15.0 h if the gas is collected in a 12.6-L container. (Assume that the products do not dissolve in chloroform.)
Using this information together with the standard enthalpies of formation of O2(g), CO2(g), and H2O(l) from...
Using this information together with the standard enthalpies of formation of O2(g), CO2(g), and H2O(l) from Appendix C, calculate the standard enthalpy of formation of acetone. Complete combustion of 1 mol of acetone (C3H6O) liberates 1790 kJ: C3H6O(l)+4O2(g)?3CO2(g)+3H2O(l)?H?=?1790kJ
Dinitrogen pentoxide (N2O5) decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition...
Dinitrogen pentoxide (N2O5) decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition is first order with a rate constant at 45 ∘C of 1.0×10−5s−1. Part A Calculate the partial pressure of O2 produced from 1.69 L of 0.524 M N2O5 solution at 45 ∘C over a period of 16.2 h if the gas is collected in a 11.6-L container. (Assume that the products do not dissolve in chloroform.) Answer Pressure in terms of atm
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT