Question 10 (5 points) ✓ SavedDetermine the standard enthalpy of reaction (AHorxn) given the enthalpies offormation below.2 Ag2S(s) + 2 H₂O(1)→ 4 Ag(s) + 2 H₂S(g) + O₂(g)AHᵒf Ag₂S(s) = -32.6 kJ/molAHᵒf H₂O(1) = -285.8 kJ/molAHᵒf Ag(s) = 0 kJ/molAHᵒf H₂S(g) = -20.6kJ/molAHᵒf O₂(g) = 0 kJ/mol30.8Il app.honorlock .com is aki

Standard enthalpy of given reaction can be find as :

Question 10 (5 points) ✓ Saved Determine the standard enthalpy of reaction (AHorxn) given the enthalpies of formation below. 2 Ag2S(s) + 2 H₂O(1)→ 4 Ag(s) + 2 H₂S(g) + O₂(g) AH Ag₂S(s) = -32.6 kJ/mol f AHᵒf H₂O(1) = -285.8 kJ/mol AHᵒf Ag(s) = 0 kJ/mol AHᵒf H₂S(g) = -20.6kJ/mol AHᵒf O₂(g) = 0 kJ/mol 30.8 N >>

Question 10 (5 points) ✓ Saved Determine the standard enthalpy of reaction (AHorxn) given the enthalpies of formation below. 2 Ag2S(s) + 2 H₂O(1)→ 4 Ag(s) + 2 H₂S(g) + O₂(g) AH Ag₂S(s) = -32.6 kJ/mol f AHᵒf H₂O(1) = -285.8 kJ/mol AHᵒf Ag(s) = 0 kJ/mol AHᵒf H₂S(g) = -20.6kJ/mol AHᵒf O₂(g) = 0 kJ/mol 30.8 N >>

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...

See similar textbooks

Similar questions

Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? endothermicexothermic (b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced? g(d) How many kilojoules of heat are released when 13.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = kJ(e) Calculate E when 360.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K kJ HopHelpCh5N1
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? exothermic endothermic (b) Calculate the amount of heat transferred when 55.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced? g(d) How many kilojoules of heat are released when 12.0 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = kJ(e) Calculate E when 450.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K
Chemistry A scientist measures the standard enthalpy change for this reaction to be -818.2 kJ/mol:Fe2O3(s) + 2 Al(s)Al2O3(s) + 2 Fe(s)Based on this value and the standard formation enthalpies for the other substances, the standard formation enthalpy of Fe2O3(s) is _____ kJ/mol.
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? endothermicexothermic (b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced? g(d) How many kilojoules of heat are released when 13.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = kJ(e) Calculate E when 360.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K kJ HopHelpCh5N1
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). thermometer stirrer First, a 6.000 g tablet of benzoic acid (C,H,C0,H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is insulation observed to rise from 13.00 °C to 40.13 °C over a time of 10.0 minutes. Next, 5.200 g of ethane (C,H) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 13.00 °C to 53.96 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H,(g) + 70,(g) 4CO,(g) + 6 H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced…
8.2
QUESTION 18 PLEASE
Using the equations determine the enthalpy for the reaction
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). thermometer stirrer First, a 5.500 g tablet of benzoic acid (C,H,CO, H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed insulation to rise from 15.00 °C to 42.56 °C over a time of 10.3 minutes. Next, 5.720 g of acetaldehyde (C2H,O} are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 15.00 °C to 40.53 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H,0(g) + 50, (g) 4CO, (g) + 4H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note…
5(a)
please I want an answer question
Consider the balanced reaction 4 A + 9 B → 8 C + 8 D and the enthalpies of formation provided in the table below. AH Compound (kJ/mol) A 170.8 231.1 D -98.4 Suppose that the AH of the overall reaction is -2,029.3 kJ/molxn. Calculate the value of the AHf of C in kJ/mol. Report your answer to three decimal places (ignore significant figures).