at 25°C, the following heats of reaction are known: 2CIF(g) + O₂(g) Ⓡ Cl₂O(g) + F₂0 2CIF3(g) + 202(g) Ⓡ Cl₂O(g) + 3F₂O(g) 2F2(g) + O₂(g) Ⓡ 2F₂O(g) DH° rxn DH° rxn = 167.4 kJ/mol = 341.4 kJ/mol DH° = -43.4 kJ/mol rxn Use Hess's law to calculate DH°rxn for the reaction: CIF(g) + F2(g) Ⓡ CIF 3(g) Express your answer in decimal notation in units of kJ with appropriate positive or negative sign, rounded to three significant figures.
at 25°C, the following heats of reaction are known: 2CIF(g) + O₂(g) Ⓡ Cl₂O(g) + F₂0 2CIF3(g) + 202(g) Ⓡ Cl₂O(g) + 3F₂O(g) 2F2(g) + O₂(g) Ⓡ 2F₂O(g) DH° rxn DH° rxn = 167.4 kJ/mol = 341.4 kJ/mol DH° = -43.4 kJ/mol rxn Use Hess's law to calculate DH°rxn for the reaction: CIF(g) + F2(g) Ⓡ CIF 3(g) Express your answer in decimal notation in units of kJ with appropriate positive or negative sign, rounded to three significant figures.
Chemistry for Engineering Students
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Chapter9: Energy And Chemistry
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Problem 9.55PAE: 9.55 Hydrogen gas will react with either acetylene or ethylene gas. The thermochemical equations for...
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Transcribed Image Text:At 25°C, the following heats of reaction are known:
2CIF(g) + O₂(g) ® Cl₂O(g) + F₂O
2CIF3(g) + 202(g) ® Cl₂O(g) + 3F₂O(g)
2F2(g) + O₂(g) Ⓡ 2F₂O(g)
DH°rxn = 167.4 kJ/mol
DH rxn
DH rxn
= 341.4 kJ/mol
= -43.4 kJ/mol
Use Hess's law to calculate DH°rxn for the reaction:
CIF(g) + F₂(g) Ⓡ CIF 3(g)
Express your answer in decimal notation in units of kJ with appropriate positive or negative sign, rounded to three significant figures.
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