Calculate the AH°, for the reaction below, in kJ, using the heat of formation values below: _X4Y2 (g) + _Z6 (g) → _X2Z4 (g) + Y4Z2 ) ---- AH°; [X4Y2 (g)] = -300.5 kJ/mol %3D AH°; [Z6 (3)] = 0 kJ/mol AH°f [X2Z4 (g)] = -110.4 kJ/mol AH°; [Y4Z2 ()] = 278.9 kj/mol HINT: Balance the reaction FIRST!

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**Calculate the ΔH°_rxn for the reaction below, in kJ, using the heat of formation values:**

\[
\text{____X}_4\text{Y}_2 \text{(g) + ____Z}_6\text{ (g)} \rightarrow \text{____X}_2\text{Z}_4 \text{(g) + ____Y}_4\text{Z}_2 \text{(l)}
\]

- ΔH°_f [X₄Y₂ (g)] = -300.5 kJ/mol
- ΔH°_f [Z₆ (g)] = 0 kJ/mol
- ΔH°_f [X₂Z₄ (g)] = -110.4 kJ/mol
- ΔH°_f [Y₄Z₂ (l)] = 278.9 kJ/mol

**HINT:** Balance the reaction FIRST!
Transcribed Image Text:**Calculate the ΔH°_rxn for the reaction below, in kJ, using the heat of formation values:** \[ \text{____X}_4\text{Y}_2 \text{(g) + ____Z}_6\text{ (g)} \rightarrow \text{____X}_2\text{Z}_4 \text{(g) + ____Y}_4\text{Z}_2 \text{(l)} \] - ΔH°_f [X₄Y₂ (g)] = -300.5 kJ/mol - ΔH°_f [Z₆ (g)] = 0 kJ/mol - ΔH°_f [X₂Z₄ (g)] = -110.4 kJ/mol - ΔH°_f [Y₄Z₂ (l)] = 278.9 kJ/mol **HINT:** Balance the reaction FIRST!
Expert Solution
Step 1

Given 

Reaction 

X4Y2(g)   +  Z6(g)    X2Z4(g)  +  Y4Z2(l)

∆H°f  [ X4Y2 (g) ]  = - 300.5 KJ/mol 

∆H°f [ Z6(g) ]   = 0 KJ/mol

∆H°f  [ X2Z4 (g) ]   = - 110.4 KJ/mol

∆H°f  [ Y4Z2 ( l ) ]  =   278.9 KJ/mol

   ∆H°( r×n ) = ? 

 

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