For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy ASn: If it's not possible to decide with the information given, check the "not enough information" button in the last column. Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction sign of reaction entropy AS < 0 rxn HCI (g) + NH, (g) → NH,CI (s) O AS pxn > 0 O not enough information, O AS < 0 rxn AgNO, (aq) + NaCI (aq) → AgCI (s) + NaNO, (aq) AS > 0 rxn O not enough information. AS < 0 rxn N, (g) + 3H, (g) - 2NH, (g) > 0 O not enough information.

For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy ASn: If it's not possible to decide with the information given, check the "not enough information" button in the last column. Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction sign of reaction entropy AS < 0 rxn HCI (g) + NH, (g) → NH,CI (s) O AS pxn > 0 O not enough information, O AS < 0 rxn AgNO, (aq) + NaCI (aq) → AgCI (s) + NaNO, (aq) AS > 0 rxn O not enough information. AS < 0 rxn N, (g) + 3H, (g) - 2NH, (g) > 0 O not enough information.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section16.3: Measuring Dispersal Of Energy: Entropy

Problem 16.3CE

See similar textbooks

Similar questions

For the process A(l) A(g), which direction is favored by changes in energy probability? Positional probability? Explain your answers. If you wanted to favor the process as written, would you raise or lower the temperature of the system? Explain.
A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 16.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate A G for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.
A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 72.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy A G of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.
What will be the Gibbs free energy in KJ/mol if the entropy of the reaction (ΔS°rxn) is 301.59 KJ/mole and the ethlapy (ΔH°rxn) is -394.59 J/mol at 27.73 oC? Answers in 2 decimal place , unit is not required.
A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 150.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.
Use the database on the textbook to calculate the entropy change of the following reaction under standard condition 1bar and 298 K: 2C2H6 (g) + 7O2 (g) = 4CO2 (g)+ 6H2O (L) ΔreactionS = _________ J/K/ (mol reaction). 4 sig. fig. per mole of reaction, not per mole of any subject. The data is copied from the appendix here material standard entropy ( J/K/mol) C2H6 229.60 O2 205.138 CO2 213.74 H2O(L) 69.91
A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 72.0 °C and constant total pressure. Then, he measures the reaction enthalpy A/ and reaction entropy AS of the first reaction, and the reaction enthalpy A/ and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.
I use dry ice (solid CO2 which is -78.5 ℃) in my lab to cool reactions. If I leave a chuck of dryice, that weights 26.3 grams on the table and the table is 25.0 ℃, and the heat ofsublimation of CO2 is 26.1 kJ/mol, what is the change in entropy of the universe, systemand surrounding if I let all of the dry ice sublime?
Benzene (C6H6) has a melting point of 5.50C and an enthalpy of fusion of 10.04kJmol-1 at 25.00C. The molar heat capacities at constant pressure for solid and liquid benzene are 100.4JK-1mol-1 and 133.0JK-1mol-1, respectively. Calculate the change of entropy of system and change of entropy of the surrounding at 100C for the reaction of C6H6(l)---->C6H6(s)
A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 60.0 °C and constant total pressure. Then, she measures the reaction enthalpy ΔH and reaction entropy ΔS of the first reaction, and the reaction enthalpy ΔH and reaction free energy ΔG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate ΔG for the first reaction and ΔS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.
For the complete neutralization reaction between a 1 M strong acid and a 1 M strong base of equal initial volumes that is marked by a temperature rise, the entropy of neutralization is positive (ΔSrxn > 0) whereas the Gibbs free energy is negative (ΔGrxn < 0). Is this true or false? Please explain.
When the oxide of generic metal MM is heated at 25.0 ∘C, a negligible amount of MM is produced. MO2(s)↽−−⇀M(s)+O2(g) Δ?∘=289.8kJmol When this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous. What is the chemical equation of this coupled process? Show that the reaction is in equilibrium. Include physical states and represent graphite as C(s)C(s). What is the thermodynamic equilbrium constant for the coupled reaction? ?=