**Thermodynamics Reaction Calculations**Enter your answer in the provided box.**Calculate ΔH°rxn for the following reaction:**\[ \text{SiO}_2(s) + 4 \text{HF}(g) \rightarrow \text{SiF}_4(g) + 2 \text{H}_2\text{O}(l) \]**Given Standard Enthalpies of Formation (ΔH°f):**- ΔH°f [SiO2 (s)] = -910.9 kJ/mol- ΔH°f [HF (g)] = -273 kJ/mol- ΔH°f [SiF4 (g)] = -1614.9 kJ/mol- ΔH°f [H2O (l)] = -285.840 kJ/mol**[Input Box for Answer]** (kJ)*Note: No graphs or diagrams are present in this text.*

Calculate enthalpy of the given reaction by using the data given--

Answered: Calculate AH for the following: rxn…

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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Q2 (a) Given that the enthalpy values for the following reactions are: AH = -1049.0 kJ 2 Al (5) + 6HCI (ад) — 2 ALCI3 (аg) + 3 Н2 (9) AH = -74.8 kJ HCl (g) → HCl (aq) + Cl2 (g) → 2HCI AH = -185.0 kJ H2 (9) + AlCl3 (s) → AlCl3 (aq) (g) AH = -323.0 kJ ΔΗ Manipulate the reactions above to determine AH for: 2 Al(s) + 3 Cl2 (9) → 2 AlCl3 (s) In one experiment, a 25 g sample of an alloy was heated to a certain temperature. (b) The heated alloy was then dropped into a beaker containing 90 g of water at 25.32 °C. The temperature of the water rose to a final value of 27.18 °C. Predict the final temperature that the alloy is being heated at the beginning of the experiment. Given that the heat capacity of water and alloy are 4.184 Jgl°C-' and 0.3847 Jg l°C' respectively.
Given the reactions, X(s) + 1/2O₂(g) XCO₂ (s) XO(s) XO(s) + CO₂(g) what is AH for this reaction? X(s) + 1/2O₂(g) + CO₂(g) AH = -763.1 kJ AH = +159.3 kJ XCO3(s)
18. From the following data, AH = -393.5 kJ/mol C(graphite) + O₂(g) → CO₂(g) 1 H₂ (g) + O₂(g) → H₂O(l) AH = -285.8 kJ/mol 2C₂H6 (g) +70₂(g) → 6H₂O(l) + 4CO₂(g) AH = -3119.06 kJ/mol calculate the enthalpy change for the reaction: 2C (graphite) (1) + 3H₂(g) → 2C₂H6 (g)
4.From these data: N2H4(l) + O2(g) à 2N2(g) + 2H2O(l) H= -622.2 kJ/mol H2(g) + ½O2 à H2O(l) H= -285.8 kJ/mol H2(g) + O2(g) à H2O2(l) H= -115 kJ/mol Find H for the reaction: N2H4(l) + 2H2O2(l) à 2N2(g) + 4H2O(l)
enon 19 of 23 For the chemical reaction Ca (s) + % O2 (g) What is the enthalpy for the reaction 2 CaO (s) → 2 Ca (s) + O2 (g)? CaO (s) AH° = -635 kJ/mol.
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04) (g Calculate the volume of air at 30°C and 1.00 atm that is needed to burn completely 10.0 grams of propane. Assume that air is 21.0 percent O₂ by volume. The heat of combustion of propane is -2,220.1 kJ/molrxn. Calculate the heat of formati of propane given that AHO of H₂0(1) = -285.3 kJ/mol and AHO of CO2(g) = -393.5 kJ/ f AH-[(3•Co₂) + (4•H₂0)]-[C3H8 + 5(0₂)] [ F)+(4(-285.3)]-[AH C3H5] [200
Given the following data, calculate the enthalpy of formation for H2O2 (AH of H202(0)) H2O2(()* O2(g) + H20(!) 2 AH = -99 kJ -> 2 H2(g) + O2(g) 2 H20(!) AH = -572 kJ
Calculate AH, (kJ/mol), enthalpy of formation, for the hypothetical CaF(s) given: AHjattice = -795 kJ/mol AHsub(Ca) = +178 kJ/mol AHje1 (Ca) = +590 kJ/mol %3D AHje2 (Ca) = +1250 kJ/mol AH(F2) = +158 kJ/mol AHea(F) = -328 kJ/mol 1053 O -974 O 874 O 974 O 1053
Given the following reactions: N2 (g) + O2 (g) → 2NO (g) AH = +180.7 kJ 2N20 (g) → O2 (g) + 2N2 (g) AH = -163.2 kJ the enthalpy of reaction for 2N20 (g) → 2NOo (g) + N2 (g) is kJ. -343.9 343.9 -145.7 145.7 O 17.5
d The standard enthalpy change for the following reaction is -602 kJ at 298 K. AH° = -602 kJ Mg(s) + 1/2O₂(g) → MgO(s) ΔΗ — What is the standard enthalpy change for the reaction at 298 K? 2 MgO(s) →→→2 Mg(s) + O₂(g) kj Submit Answer Retry Entire Group 9 more group attempts remaining
6. Calculate the AH for the reaction: 7. CS2 (1) + 2 O2 (g) → CO2 (g) + 2 SO2 (g) Given: AHCO2 (g) = - 393.5 kJ/mol; AHSO2 = -296.8 kJ/mol; %3D AHCS2 (1) = 87.9kJ/mol

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Calculate AH for the following: rxn SiO2(s) + 4 HF(g) SiF (g) + 2 H,0() AH (SIO2 (s)]=-910.9 kJ/mol AH HF (g)] =-273 kJ/mol %3D AH [SIF (g)] =-1,614.9 kJ/mol f AH H O (1)] =-285.840 kJ/mol f kJ