**Problem 61:** For each reaction, calculate ΔH°_rxn, ΔS°_rxn, and ΔG°_rxn at 25 °C and state whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 °C? a. \( \text{N}_2\text{O}_4(g) \rightarrow 2 \text{NO}_2(g) \) b. \( \text{NH}_4\text{Cl}(s) \rightarrow \text{HCl}(g) + \text{NH}_3(g) \) c. \( 3 \text{H}_2(g) + \text{Fe}_2\text{O}_3(s) \rightarrow 2 \text{Fe}(s) + 3 \text{H}_2\text{O}(g) \) d. \( \text{N}_2(g) + 3 \text{H}_2(g) \rightarrow 2 \text{NH}_3(g) \) **Instructions:** - Calculate the enthalpy change (ΔH°_rxn) for each reaction.- Calculate the entropy change (ΔS°_rxn) for each reaction.- Calculate the Gibbs free energy change (ΔG°_rxn) at 25 °C for each reaction.- Determine if each reaction is spontaneous under standard conditions at 25 °C.- For non-spontaneous reactions, assess if a temperature change could facilitate spontaneity and recommend whether the temperature should be raised or lowered.

a. The reaction: N₂O₄(g) → 2 NO₂(g) Standard enthalpies of formation: N₂O₄(g): Hf =…

For each reaction, calculate AHrn, ASn, and AGxn at 25 °C and state whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 °C? a. N2O4(8) – 2 NO2(g) b. NH4C1(s) c. 3 H2(8) + Fe2O3(s) → 2 Fe(s) + 3 H2O(8) d. N2(8) + 3 H2(8) 0.25 HCl(8) + NH3(8) - | 2 NH3(8) HO

For each reaction, calculate AHrn, ASn, and AGxn at 25 °C and state whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 °C? a. N2O4(8) – 2 NO2(g) b. NH4C1(s) c. 3 H2(8) + Fe2O3(s) → 2 Fe(s) + 3 H2O(8) d. N2(8) + 3 H2(8) 0.25 HCl(8) + NH3(8) - | 2 NH3(8) HO

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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Indicate whether each statement is true or false. All spontaneous processes are fast.
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49.For the decomposition of hydrogen peroxide to water and oxygen, H2O2(g) ⟶⟶ H2O(g) + O2(g) ΔΔH° = -106 kJ, and ΔΔS° = +0.0580 kJ/K. In what temperature range is the reaction spontaneous (ΔΔG° < 0)? A. The temperature must be greater than 1.83××103 K B. The temperature must be less than 1.83 ××103 K. C. The temperature must be between 225 K and 1.83 ××103 K. D. ΔΔG° is always less than zero. E. ΔΔG° is never less than zero.
For each reaction, calculate ΔH°rxn, ΔS°rxn, and ΔG°rxn at 25 °C and state whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 °C?a. 2 CH4( g)------->C2H6( g) + H2( g)b. 2 NH3( g)------> N2H4( g) + H2( g)c. N2( g) + O2( g)-------->2 NO( g)d. 2 KClO3(s)-------->2 KCl(s) + 3 O2( g)
47. Fill in the blanks in the table. Both AH and AS refer to the system. MISSED THIS? Read Section 19.60; Watch KCV 19.60 ΔΗ + AS + + AG Temperature dependent Low Temperature Spontaneous High Temperature Spontaneous Nonspontaneous Nonspontaneous