Exothermic reactions _________. Group of answer choices release heat to the surroundings. lose free energy to the surroundings. are always spontaneous. are always spontaneous and lose free energy to the surroundings

Consider the following thermodynamic table. Ca(OH)2 (s) Ca²+ (aq) S (J/mol-K) Hf (kJ/mol) Gf (kJ/mol) OH(aq) 83.4 -53.1 -10.8 -986.1 -542.8 -230.0 -898.6 -553.6 -157.2 Which of the following statements is correct with respect to the reaction Ca(OH)2 (s) = Ca2+ (aq) + 2 OH¯ (aq) ? O a) The reaction is exothermic. The solubility of calcium hydroxide will increase with increasing temperature. Ob) The reaction is endothermic. The solubility of calcium hydroxide will increase with increasing temperature. c) The reaction is endothermic. The solubility of calcium hydroxide will decrease with increasing temperature. d) The reaction is exothermic. The solubility of calcium hydroxide will decrease with increasing temperature.

Determine if the temperature will increase, decrease, or remain the same for each of the following situations. Temperature of the surroundings in an exothermic reaction. v Choose... Decreases Temperature of the surroundings in an endothermic reaction Remain the same on Temperature of the system in an endothermic reaction. Increases Temperature of the system in an exothermic reaction. Choose... MacBook Pro G Search or type URL & $ % 6 8. 2 3 4

Circle the substance in each pair that is LOWER INTERNAL ENERGY, then briefly state the chemical principle that describes WHY that substance is lower in energy.

1. A potential chemical reaction at 25.0 °C has a ΔHrxn of 147.5 kJ and a ΔSrxn of -386.9 J/K. What is the ΔGrxn in kJ.  (Enter answer to 3 significant figures and include no units in your answer) Also, what is true about the potential reaction in the previous problem? a. spontaneous b. illegal c. combustive d. nonspontaneous

Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change An exothermic chemical reaction between a solid and a liquid results in gaseous products. A solid precipitates from a solution, absorbing heat as it does so. A gas expands, absorbing heat from its surroundings. Is this change spontaneous? Yes. No. Can't decide with information given. Yes. No. O Can't decide with information given. Yes. No. Can't decide with information given. X

Explain each of the Laws of Thermodynamics and to which law would Entropy and Enthalpy apply. Thank you!

4. A particular endothermic process results in an decrease in system entropy; therefore, the G value is _________ and the process is _____________. a. negative; spontaneous b. negative; nonspontaneous c. positive; spontaneous  d. positive; nonspontaneous

One mole of an ideal gas is contained in a cylinder with a movable piston. The temperature is constant at 77°C. Weights are removed suddenly from the piston to give the following sequence of three pressures. a. P, = 4.60 atm (initial state) b. P₂ = 2.73 atm c. P3 1.00 atm (final state) What is the total work (in joules) in going from the initial to the final state by way of the preceding two steps? J What would be the total work if the process were carried out reversibly?

1.) Complete A and B to move on. a.) Write the complete, balanced chemical equation for the following reaction on a separate sheet of paper. Provide products where they are not given. Assume that the reaction is spontaneous. Propane (C3H8) + oxygen → carbon dioxide + water Type the sum of the coefficients in the equation into the answer blank.  If there is no coefficient, count it as one. Include ( g, s, l, or aq) b.) Write the complete, balanced chemical equation for the following reaction on a separate sheet of paper. Provide products where they are not given. Assume that the reaction is spontaneous. Diphosphorus pentoxide + water → Type in the coefficient and formula for the product in the equation that contains phosphorus. Include ( g, s, l, or aq)