54. Remember the enthalpy of reaction can be obtained from the enthalpy of formations. (The formula is on the equations page!)Given the enthalpy of formation of each of the following:SiO2 (s) delta Hf = - 910.9 kJ/molSİF4 (g) delta Hf = – 1614.9 kJ/molHF (g)delta Hf= - 273 kJ/molFind the enthalpy of reaction for the reaction:SİF4 (g) + O2 (g) + 2 H2 (g) → SiO2 (s) + 4 HF (g)delta Hrxn?Select one:a. – 2799 kJb. none of theseC. + 2003 kJd. + 431 kJe. + 18.3 kJf. – 388 kJg. – 431 kJh. + 2799 kJi. + 388 kJj. – 2003 kJ

∆Hrxn = ∆Hproducts - ∆Hreactants .

Given the enthalpy of formation of each of the following: SiO2 (s) delta Hf = - 910.9 kJ/mol SIF4 (g) delta Hf = - 1614.9 kJ/mol HF (g) delta Hf = - 273 kJ/mol Find the enthalpy of reaction for the reaction: SİF4 (g) + O2 (g) + 2 H2 (g) → SiO2 (s) + 4 HF (g) delta Hrxn = ? Select one: a. – 2799 kJ b. none of these C. + 2003 kJ d. + 431 kJ e. + 18.3 kJ f. – 388 kJ g. – 431 kJ h. + 2799 kJ i. + 388 kJ O j.- 2003 kJ

Given the enthalpy of formation of each of the following: SiO2 (s) delta Hf = - 910.9 kJ/mol SIF4 (g) delta Hf = - 1614.9 kJ/mol HF (g) delta Hf = - 273 kJ/mol Find the enthalpy of reaction for the reaction: SİF4 (g) + O2 (g) + 2 H2 (g) → SiO2 (s) + 4 HF (g) delta Hrxn = ? Select one: a. – 2799 kJ b. none of these C. + 2003 kJ d. + 431 kJ e. + 18.3 kJ f. – 388 kJ g. – 431 kJ h. + 2799 kJ i. + 388 kJ O j.- 2003 kJ

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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