acU3(S) decomposes lhto (S) and CO21g) at 1 atm the air around the reaction decreases in temperature. Rxn: CaCO3(s) → CaO(s) + CO2(g) Which statement is true about the decomposition of CaCO3(s) into CaO(s) and CO2(g) at 1.00 atm? The reaction is spontaneous at low temperatures. The reaction is spontaneous at all temperatures. The reverse reaction is spontaneous at all temperatures.

acU3(S) decomposes lhto (S) and CO21g) at 1 atm the air around the reaction decreases in temperature. Rxn: CaCO3(s) → CaO(s) + CO2(g) Which statement is true about the decomposition of CaCO3(s) into CaO(s) and CO2(g) at 1.00 atm? The reaction is spontaneous at low temperatures. The reaction is spontaneous at all temperatures. The reverse reaction is spontaneous at all temperatures.

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

8.
Consider a reaction that has a negative AH and a negative AS. Which of the following statements is TRUE? A) This reaction will be nonspontaneous at all temperatures. B) This reaction will be spontaneous at all temperatures. C) This reaction will be nonspontaneous only at high temperatures. D) This reaction will be spontaneous only at high temperatures. E) It is not possible to determine without more information. Given the following equation, N20(g) + NO2(g) → 3 NO(g) AG°rxn = - 23.0 kJ Determine AG°rn for the following reaction. 3 NO(g) → N20(g) + NO2(g) A) -69.0 kJ B) -23.0 kJ C) 69.0 kJ D) -7.67 kJ E) 23.0 kJ
For the reaction: 2 Cu(s) + 12 O2(g) → Cu₂O(s) AG° = -141 kJ/mol. What is the free energy change (AG) when the reaction is conducted at 327 °C using 10.0 atm of O₂(g)?
For a specific reaction, AH = -25.8 kJ/mol and AS = +45.6 J/K-mol. Which of these statements is true? O The reaction is never spontaneous. O The reaction is only spontaneous at high temperatures. OThe reaction is spontaneous at all temperatures. The reaction is only spontaneous at low temperatures.
When ∆G is negative, a chemical reaction is spontaneous non-spontaneous endothermic exothermic
17
For the reaction 2NO(g) + O2(g) → 2NO2(g), AH° = -113.1 kJ/mol and AS° = -145.3 J/K-mol. Under which temperature conditions would the reaction be spontaneous? Only at low temperatures Not possible to be spontaneous at all temperatures Only at high temperatures For all temperatures
Consider the following reaction
For each reaction with ΔH = + 245 kJ/mol and ΔS = + 48 J/molK ,at what temperature at which the reaction will be spontaneous.
The following reaction takes place at 120°C: H20( I) → H20( g) AH 44.0 kJ/ mol AS = 0.119 kJ/mol K Which of the following must be true? O a. The reaction is not spontaneous. b. The reaction is spontaneous. O c. AG = 0 O d. AG <0 O e. Two of these.
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)