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Examples of Ionic Compounds

22. The heat ...

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22. The heat of formation (N2O5,g) in KJ/mol on the bases of the following data is 2NO(g)+O2(g)---->2NO2(g) H= -114kJ/mol 4NO2(g)+O2(g)--->2N2O5(g) H= -102.6KJ/mol Heat of formation (NO,g)= 90.2 kJ/mol 1)15.1 2)30.2 3)-36.2 4 none of these

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Q. Compute the heat of formation of liquid methyl alcohol in kilojoules per mole using the following data.
The heat of vaporisation of liquid methyl alcohol =

38 k J / m o l

.
The heats of formation of gaseous atoms from the elements is their standard states:

H, 218 k J / m o l

C, 713 k J / m o l

O, 249 k J / m o l

.
Average bond energies:

C - H = 415 k J / m o l

C - O = 365 k J / m o l

O - H = 463 k J / m o l

.

Q. Compute the heat of formation of liquid methyl alcohol (in kJ mol

^{- 1}

) using the following data. The heat of vaporisation of liquid methyl alcohol is 38 kJ mol

^{- 1}

The heat of formation of gaseous atoms from the elements in their standard states:

H =

^{- 1}

C = 715

^{- 1}

O = 249

^{- 1}

Average bond energies:

C - H = 415

^{- 1}

C - O = 356

^{- 1}

O - H = 463

^{- 1}

Q. What is the heat of formation of liquid methyl alcohol in

k J m o l^{- 1},

use the following data.
Heat of vaporization of liquid methyl alcohol =

38 k J m o l^{- 1}

.
Heat of formation of gaseous atoms from the elements in their standard states:

H = 218 k J m o l^{- 1}, C = 715 k J m o l^{- 1}, O = 249 k J m o l^{- 1}

Average bond energies :

C - H = 415 k J m o l^{- 1} C - O = 356 k J m o l^{- 1} O - H = 463 k J m o l^{- 1}

Q. Compute the heat of formation of liquid methyl alcohol in kilojoules per mole using the following data.
The heat of vaporisation of liquid methyl alcohol =

38 k J / m o l

.
The heats of formation of gaseous atoms from the elements in their standard states:

H, 218 k J / m o l

C, 715 k J / m o l

O, 249 k J / m o l

.
Average bond energies:

C - H = 415 k J / m o l

C - O = 365 k J / m o l

O - H = 463 k J / m o l

.

Q. Given the following:

C (s) + O_{2} (g) \to C O_{2} (g); Δ H = - 394 k J / m o l

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l); Δ H = - 568 k J / m o l

C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l); Δ H = - 1058 k J / m o l

Using the given data, the heat of formation of ethanol is:

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