Solution Found!
Calculate for each of the following:(a) SiO2(s) + 4HF(g) ?
Chapter 5, Problem 54P(choose chapter or problem)
Calculate \(\Delta \mathrm{H}^{\circ}{ }_{\mathrm{rxn}}\) for each of the following:
\(\mathrm{SiO}_{2}(\mathrm{~s})+4 \mathrm{HF}(\mathrm{g}) \rightarrow \mathrm{SiF}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{I})\)
\(\mathrm{C}_{2} \mathrm{H}_{0}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CO}_{4}(\mathrm{l})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) [unbalanced]
Equation Transcription:
H°rxn
SiO2(s) + 4HF(g) SiF2(g) + 2H2O(I)
C2H6(g) + O2(g) CO4(l) + H2O(g)
Text Transcription:
Delta H°_rxn
SiO_2(s) + 4HF(g) rightarrow SiF_2(g) + 2H_2O(I)
C_2H_6(g) + O_2(g) rightarrow CO_4(l) + H_2O(g)
Questions & Answers
QUESTION:
Calculate \(\Delta \mathrm{H}^{\circ}{ }_{\mathrm{rxn}}\) for each of the following:
\(\mathrm{SiO}_{2}(\mathrm{~s})+4 \mathrm{HF}(\mathrm{g}) \rightarrow \mathrm{SiF}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{I})\)
\(\mathrm{C}_{2} \mathrm{H}_{0}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CO}_{4}(\mathrm{l})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) [unbalanced]
Equation Transcription:
H°rxn
SiO2(s) + 4HF(g) SiF2(g) + 2H2O(I)
C2H6(g) + O2(g) CO4(l) + H2O(g)
Text Transcription:
Delta H°_rxn
SiO_2(s) + 4HF(g) rightarrow SiF_2(g) + 2H_2O(I)
C_2H_6(g) + O_2(g) rightarrow CO_4(l) + H_2O(g)
ANSWER:
Solution 54P
Here we have to calculate for each of the following:
Step 1
(a) SiO2(s) + 4HF(g) → SiF4(g) + 2H2O(l)
The enthalpy of reaction is defined as the () difference between sum of the standard enthalpy of product and the reactant.
=
-
= {[SiF4 (g)] + 2
[H2O (l)] }- {
[SiO2 (s)] + 4
[HF(g)] }
= [(-1614.9 kJ/mol) + 2 (-285.8 kJ/mol)] - [ (-910.9 kJ/mol) + 4 (-273.0)]
= 959.6 kJ
Thus the heat of reaction is found to be 959.6 kJ.