Question

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

Homework Answers

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 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
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...
Use the data below to determine the standard molar enthalpy of formation of B2H6 (g). 4B(s)...
Use the data below to determine the standard molar enthalpy of formation of B2H6 (g). 4B(s) + 3 O2(g) --> 2 B2O3................................deltaHrxn= -2543.9 kj/mol H2(g) + 1/2 O2(g) --> H2O(g).............................deltaHrxn= -241.8 kj/mol B2H6(g) + O2(g) --> B2O3(s) + 3 H2O(g)..........deltaHrxn= -2032.9kj/mol
The standard molar enthalpy of formation, of diborane cannot be determined directly because the compound cannot...
The standard molar enthalpy of formation, of diborane cannot be determined directly because the compound cannot be prepared by reaction of boron and hydrogen. However, the value can be calculated. Calculate the standard enthalpy of formation of gaseous diborane(B2H6) using the following thermochemical information: i) 4B(s) + 3O2(g) --> WB2O3(S) = -2509.1kJ ii) 2H2(g) + O2(g) --> 2H2O(l) = - 571.7kJ iii) B2H6(g) + 3O2(g) --> B2O3(s) + 3H2O(l) = -2147.5 kJ
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
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)
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
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
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT