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MR
Test #1 - Energetics
Assigned to Guests
by Trudy Jackson
Live Session
4 Questions

1
5
Calculate the standard enthalpy of formation of gaseous diborane (B2H6) using the following thermochemical information:
4B (s) + 3O2 (g)
→\rightarrow
→ 2B2O3 (s);
Δ\Delta
Δ H = -2509.1 kJ
2H2 (g) + O2 (g)
→\rightarrow
→ 2H2O (l);
Δ\Delta
Δ H = -571.7 kJ
B2H6 (g) + 3O2 (g)
→\rightarrow
→ B2O3 (s) + 3H2O (l);
Δ\Delta
Δ H = -2147.5 kJ
(click below to write/draw)

=

B2H6(G)

2B(S)+3H2
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2
5
Hydrogen cyanide can be prepared by the reaction:

CH4 (g) + NH3 (g)
→\rightarrow
→ HCN (g) + 3H2 (g)

What is the heat of reaction at constant pressure? Use the following thermochemical equations:

N2 (g) + 3H2 (g)
→ \rightarrow
→ 2NH3 (g);
Δ\Delta
Δ H = -91.8 kJ
C (graphite) + 2H2 (g)
→\rightarrow
→ CH4 (g);
Δ\Delta
Δ H = -74.9 kJ
H2 (g) + 2C (graphite) + N2 (g)
→\rightarrow
→2HCN (g);
Δ \Delta
Δ H = 270.3 kJ

(click below to write/draw)

3
5
Complete the following Born Haber cycle for barium phosphide, Ba3P2.
(click below to write/draw)

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4
5
Use bond energies to estimate
Δ\Delta
ΔH for the reaction below:
(click below to write/draw)

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Hydrogen cyanide can be prepared by the reaction:

CH4 (g) + NH3 (g)
→\rightarrow
→ HCN (g) + 3H2 (g)

What is the heat of reaction at constant pressure? Use the following thermochemical equations:

N2 (g) + 3H2 (g)
→ \rightarrow
→ 2NH3 (g);
Δ\Delta
Δ H = -91.8 kJ
C (graphite) + 2H2 (g)
→\rightarrow
→ CH4 (g);
Δ\Delta
Δ H = -74.9 kJ
H2 (g) + 2C (graphite) + N2 (g)
→\rightarrow
→2HCN (g);
Δ \Delta
Δ H = 270.3 kJ