**Question 5 of 26****Determine the Enthalpy for the Reaction**Using the provided table, determine the enthalpy for the reaction:\[ \text{C}_3\text{H}_8 \, (g) + 5 \, \text{O}_2 \, (g) \rightarrow 3 \, \text{CO}_2 \, (g) + 4 \, \text{H}_2\text{O} \, (g) \]**Table: Standard Enthalpies of Formation**| Substance | \( \Delta H_f^\circ \) (kJ/mol) ||-----------|--------------------|| \(\text{C}_3\text{H}_8 \, (g)\) | -108.4 || \(\text{O}_2 \, (g)\) | 0 || \(\text{CO}_2 \, (g)\) | -393.5 || \(\text{H}_2\text{O} \, (g)\) | -241.8 |This table lists the standard enthalpies of formation for each substance involved in the chemical reaction. The values are given in kilojoules per mole (kJ/mol). This information is critical in calculating the overall change in enthalpy for the chemical reaction using Hess's Law.

The difference between the heat of formation of product to the heat of formation of reactant is…

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Using the provided table, determine the enthalpy for the reaction C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (g) Substance AH¡ (kJ/mol) CэНв (9) -108.4 O2 (g) CO2 (g) -393.5 H2O (g) -241.8

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Using the provided table, determine the molar enthalpy (in kJ/mol) for the reaction 2 NH3(g) + 3 N₂O (g)→ 4 N₂ (g) + 3 H₂O (1) Substance NH3 (9) N₂O (g) N₂ (g) H₂O (1) AHf (kJ/mol) -46.2 81.6 0 -285.8
Given the standard enthalpy changes for the following two reactions: (1) 2C(s) + 2H2(g) C2H4(g) AH° = 52.3 kJ (2) 2C(s) + 3H2(g) C2H6(g) AH° = -84.7 kJ what is the standard enthalpy change for the reaction: (3) C2H4(g) + H2(g) C2H6(g) AH° = ? kJ
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Determine the enthalpy change, AH, in kJ, for the following reaction: CS2 (1) + 302 (g) --> CO₂ (g) + 2SO2 (g) given the following thermochemical equations: C(s) + O₂ (g) --> CO₂ (g) ΔΗ = 91.2 kJ S (s) + O₂ (g) --> SO₂ (g) ΔΗ = -382 kJ C(s) + 2S (g) --> CS₂ (1) Do not report units in your answer. Report your answer to one decimal place and include the correct sign in your answer. AH = 82.6 kJ
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Use Hess’s law to calculate the enthalpy change for the reaction WO3(s) + 3H2(g) —> W(s) +3H2O(g) from the following data: 2W(s) + 3O2(g) —> 2 WO3(s) H=-1685.4 2H2(g) + O2(g) —> 2H2O(g) H=-477.84
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Using standard heats of formation, calculate the standard enthalpy change for the following reaction. 2HBr(g) + Cl₂(g) → 2HCl(g) + Br₂(g) AH (HBr(g)) = -36.3 kJ/mol AH (Cl₂ (9)) = 0.0 kJ/mol AH (HCl(g)) = -92.3 kJ/mol AH (Br₂ (9)) = 30.9 kJ/mol AH rxn = kJ
Find the standard change in enthalpy for the following reaction. N₂H4(1) + O₂(g) → 2 NO(g) + 2 H₂O(g) Given the following known reactions: N₂(g) + 2 H₂(g) → N₂H₁ AH = 97.4 kJ/mol N₂(g) + O₂(g) → NO(g) AH = 90.2 kJ/mol H₂(g) + O₂(g) → H₂O(g) AH = -242 kJ/mol Remember you need to include O₂ to get a balanced reaction but its AH = 0 kJ/mol !!
1) From the following data, C(graphite) + O2(g) à CO2(g) = -393.5 kJ/mol H2(g) + 1/2O2(g) = H2O(l) delta H = -285.8 kJ/mol 2C2H6(g) + 7O2(g) = 4CO2(g) + 6H2O(l) delta H = -3119.6 kJ/mol calculate the enthalpy change for the reaction 2C(graphite) + 3H2(g) =C2H6(g) a) –2417.2 kJ b) –84.6 kJ c) 2417.2 kJ d) –3204.2 kJ
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（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g) ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A? （2）Consider the reaction: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?