Chemical Thermodynamics Quiz

<p>ΔG becomes less negative or positive. (B)</p> Signup and view all the answers

<p>−100 kJ/mol (C)</p> Signup and view all the answers

<p>Phase change from solid to liquid (C)</p> Signup and view all the answers

<p>Condensation of water vapor (D)</p> Signup and view all the answers

<p>The number of energetically equivalent arrangements possible (D)</p> Signup and view all the answers

<p>It increases (C)</p> Signup and view all the answers

<p>ΔS = +, because the number of particles increases (C)</p> Signup and view all the answers

<p>W (B)</p> Signup and view all the answers

<p>Solids have the highest degree of organization (A)</p> Signup and view all the answers

<p>Increases the entropy (C)</p> Signup and view all the answers

<p>16 (C)</p> Signup and view all the answers

<p>It increases to 16 (A)</p> Signup and view all the answers

<p>The most probable macrostate contains the highest number of microstates. (C)</p> Signup and view all the answers

<p>1 (D)</p> Signup and view all the answers

<p>6 (A)</p> Signup and view all the answers

<p>A in top left, B in bottom area (D)</p> Signup and view all the answers

<p>Microstates increase and macrostates increase. (C)</p> Signup and view all the answers

<p>Each macrostate can be represented by multiple microstates. (A)</p> Signup and view all the answers

<p>99.1 J/mol・K (A)</p> Signup and view all the answers

<p>620 K (D)</p> Signup and view all the answers

<p>-457.1 kJ (C)</p> Signup and view all the answers

<p>T (B)</p> Signup and view all the answers

<p>ΔG = ΔG° + RT ln Q (C)</p> Signup and view all the answers

<p>It is the gas constant. (C)</p> Signup and view all the answers

<p>Combustion of propane (C)</p> Signup and view all the answers

<p>By subtracting the enthalpy of Hg(g) from that of Hg(l) (C)</p> Signup and view all the answers

<p>−200 kJ (D)</p> Signup and view all the answers

<p>ΔGrxn° = Σ m[ΔGf°(products)] - Σ n[ΔGf°(reactants)] (B)</p> Signup and view all the answers

<p>0 kJ/mol (D)</p> Signup and view all the answers

<p>The free-energy change upon formation from standard states (C)</p> Signup and view all the answers

<p>ΔS° (B)</p> Signup and view all the answers

<p>-49.5 kJ/mol (D)</p> Signup and view all the answers

<p>The reaction is spontaneous in the forward direction. (D)</p> Signup and view all the answers

<p>13.24 (C)</p> Signup and view all the answers

<p>K = e^(ΔG° / RT) (A)</p> Signup and view all the answers

<p>5.6 x 105 (D)</p> Signup and view all the answers

<p>The equilibrium pressures of both reactants and products (C)</p> Signup and view all the answers

<p>The reaction quotient (B)</p> Signup and view all the answers

<p>365 K (A)</p> Signup and view all the answers

A measure of disorder or randomness in a system.

Entropy increases in a chemical process.

Entropy decreases in a chemical process.

Entropy increases. A solid becomes less ordered in liquid form.

Entropy increases. Particles become much more disordered in the gas phase.

Entropy increases. Increased kinetic energy means more ways the particles can move.

Energetically equivalent ways to arrange components in a system

A constant that relates entropy (S) to the number of microstates (W).

W = X^n, where X is the number of locations, and n is the number of particles.

The macrostate with the largest number of microstates.

Example: 4 possible locations for 2 particles.

Calculation of possible arrangements when the divider is removed.

Different arrangements like particles together or separate.

The change in Gibbs free energy when one mole of a compound is formed from its elements in their standard states at 298 K and 1 atm.

The change in Gibbs free energy during a chemical reaction under standard conditions (298 K and 1 atm).

We can calculate the Gibbs free energy change of a reaction by subtracting the sum of the standard Gibbs free energy of formation values of the reactants from the sum of the standard Gibbs free energy of formation values of the products, multiplied by their respective stoichiometric coefficients.

A reaction that occurs without external energy input and proceeds in the direction of decreasing Gibbs free energy (ΔG < 0).

We can calculate Gibbs free energy at temperatures other than 298 K using the equation: ΔG = ΔH° – TΔS°, where ΔH° and ΔS° are standard enthalpy and entropy changes.

The maximum amount of useful work (non-expansion work) a system can perform at constant temperature and pressure.

Conditions in a reaction where the reactants and products are not at their standard state (1 atm pressure, 298 K). This affects the Gibbs Free Energy change.

A measure of the relative amount of reactants and products at a given time during a reaction. It helps predict the direction of the reaction to reach equilibrium.

ΔG = ΔG° + RT ln Q

A thermodynamic potential that measures the amount of useful work obtainable from a thermodynamic system at a constant temperature and pressure.

The change in free energy that occurs when 1 mole of a compound is formed from its elements in their standard states.

The change in free energy that occurs during a chemical reaction under standard conditions.

DG°rxn = å m[DG°f (products)] - å n[DG°f (reactants)]

A reaction that requires external energy input to occur and absorbs free energy.

A negative DG°rxn indicates a spontaneous reaction and a positive DG°rxn indicates a non-spontaneous reaction.

The combustion of propane is a spontaneous reaction with a negative DG°rxn because it releases energy.

The Gibbs free energy change of a reaction under standard conditions (298 K and 1 atm pressure).

A constant that describes the ratio of products to reactants at equilibrium.

ΔG = -RT ln K (where R is the gas constant and T is the temperature in Kelvin).

A state where the rates of the forward and reverse reactions are equal, and the net change in concentrations is zero.