Lab: Calorimetry and Specific Heat — Unit test Answers

Which process involves a decrease in entropy?

Examine the following processes.i. Glucose breaks down in our bodies to provide energy.ii. A lump of sugar dissolves in a cup of coffee.iii. A candle burns.iv. Ice cream melts on a hot day.v. Food is refrigerated in a refrigerator.vi. A drop of food coloring spreads in a glass of water.Which arrangement correctly categorizes the above processes into either spontaneous or nonspontaneous processes?

This is the equation for the dissociation of ammonia gas at 293 K. H = 145 kJ and S = 195 J/k.2NH3(g) N2(g) + 3H2(g) Which correctly states the G for this dissociation and whether the process is spontaneous or nonspontaneous? Use G = H – TS.

Which process is spontaneous?

Which process involves an increase in entropy?

Which statement describes spontaneous processes?

Which statement describes a system that consists of sugar crystals dissolving in water?

The reaction below proceeds spontaneously at 298 K. NH3(g) +Cl2(g)NH4Cl(s)What is the sign of the entropy change, S?

Consider the reaction 2SO2(g) + O2(g) 2SO3(g).SubstanceHf (kJ/mol)S (J/(molK))SO3(g)–396130.58SO2(g)–297191.50O2(g)0205.00What is the Grxn of this reaction, and would it be spontaneous or nonspontaneous at 300.0 K? Use G = H – TS.

Which process or processes produce an increase in entropy?i. N2(g) + 3H2(g) NH3(g)ii. C10H8(g) C10H8(s)iii. CH3OH(l) CH3OH(aq)