Consider the decomposition of liquid water, H₂O(l):(a) What is the enthalpy change for the reverse reaction?AHreverse -205.9X kJ/mol.H₂O(1) H₂(g) + 1/2 O₂(g)(b) Balance the forward reaction with whole-number coefficients. What is AH for the reaction represented by this equation?ΔΗ = 541.0X kJ/mol.AH should increaseAH = 285.9 kJ(c) which is more likely to be thermodynamically-favored, the forward reaction or the reverse reaction?The forward reaction. ✔ X(d) If the (forward) reaction were written to consume water gas, H₂O(g), instead of liquid water, would you expect themagnitude of AH to increase (become more positive), decrease (become more negative), or stay the same?X

Given reaction of the decomposition of liquid water is H2O (l) <=======> H2(g) + 1/2 O2(g)…

Consider the decomposition of liquid water, H₂O(1): (a) What is the enthalpy change for the reverse reaction? AHreverse = -205.9 x kJ/mol. H₂O(1) H₂(g) + 1/2 O₂(g) (b) Balance the forward reaction with whole-number coefficients. What is AH for the reaction represented by this equation? ΔΗ = |541.0 x kJ/mol. ΔΗ = 285.9 kJ (c) Which is more likely to be thermodynamically-favored, the forward reaction or the reverse reaction? The forward reaction. ✔ X AH should increase (d) If the (forward) reaction were written to consume water gas, H₂O(g), instead of liquid water, would you expect the magnitude of AH to increase (become more positive), decrease (become more negative), or stay the same? X

Consider the decomposition of liquid water, H₂O(1): (a) What is the enthalpy change for the reverse reaction? AHreverse = -205.9 x kJ/mol. H₂O(1) H₂(g) + 1/2 O₂(g) (b) Balance the forward reaction with whole-number coefficients. What is AH for the reaction represented by this equation? ΔΗ = |541.0 x kJ/mol. ΔΗ = 285.9 kJ (c) Which is more likely to be thermodynamically-favored, the forward reaction or the reverse reaction? The forward reaction. ✔ X AH should increase (d) If the (forward) reaction were written to consume water gas, H₂O(g), instead of liquid water, would you expect the magnitude of AH to increase (become more positive), decrease (become more negative), or stay the same? X

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? 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
When methanol, CH, OH, is burned in the presence of oxygen gas, O,, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH, OH(g) + 0,(g) → CO,(g) + 2 H,O(1) ΔΗ --764 kJ How much methanol, in grams, must be burned to produce 837 kJ of heat?
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
31
How many grams of CaO must be added to 50.0 mL of water to make the temperature increase from 25.0 Â°C to 58.87 Â°C? The reaction is CaO(s) + H 2O(l) ↔ Ca(OH) 2(aq) -- ΔH = -83.7 kJAssume the heat capacity of the solution is the same as pure water (4.184 J/g*Â°C), the density of the solution is 1.00 g/mL and there is no loss of heat to the surroundings.
27. When 0.0500 mol of CH4 (g) burns, 40.1 kJ of heat is produced. What is the change in enthalpy (AH) in kJ for the following reaction: CH4 (g) (a) +802 kJ/mol + 202 (g) (b) -802 kJ/mol , CO₂ (g) + 2H₂O(g) + Heat (c) +40.1 kJ/mol (d) -40.1 kJ/mol
Given the standard enthalpy changes for the following two reactions: (1) N2(g) + 202(g)N204(g) AH° = 9.2 kJ (2) 2N20(g)2N2(g) + O2(g) AH° = -164.2 kJ what is the standard enthalpy change for the reaction: (3) 2N½0(g) + 302(g)- →2N2O4(g) AH° = ? kJ
（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?
8. The oxidation of the sugar glucose, C6H1206 is described by the following equation: C6 H12 06 (s) + 602 (g) → 6CO2 (g) + 6H2 O(1) AH=-2816 kJ The metabolism of glucose gives the same products, although the glucose reacts with oxygen in a series of steps in the body. (a) How much heat in kilojoules can be produced by the metabolism of 1.0 g of glucose? (b) How many Calories can be produced by the metabolism of 1.0 g of glucose? Dags 1 of 514 words 170
In a coffee cup calorimeter, 3.00 g of NaOH (molar mass 40.00g/mol) was mixed with 75.0 mL of 1.00M HNO3. If the initial temperature of the HNO3 was 31.3°C and the final temperature of the solution was 22.3°C, determine AH for the reaction in kJ/mol. NaOH(s) + HNO3(aq) ===> NaNO3(aq) + H2O) The density and the specific heat capacity of the resulting solution are 1.00 g/ml and 4.18 J/°C.g, respectively. Units do not need to be typed, simply enter the correct number. If the sign of AH is negative put a negative sign (-) in the answer. Answer: