1. State the first and second laws of thermodynamics

9.11 Analyze the units of the quantity (pressurevolume) and show that they are energy units, consistent with the idea of PV-work.

What are the two ways that a final chemical state of a system can be more probable than its initial state?

The second law of thermodynamics is sometimes paraphrased as: you can't break even. Explain. Because energy cannot be created out of nothing. Because some energy is lost in all energy transactions. Because some energy is gained in all energy transactons.

• define state functions and explain their importance.

A pot of cold water is heated on a stove, and when the water boils, a fresh egg is placed in the water to cook. Describe the events that are occurring in terms of the zeroth law of thermodynamics.

Explain why absolute enthalpies and energies cannot be measured, and only changes can be determined.

Starting with equation 2.27 andthe original definitionof enthalpy, derive the fact that Cp-=Cv-+R

The reaction SO3(g)+H2O(l)H2SO4(aq) is the last step in the commercial production of sulfuric acid. The enthalpy change for this reaction is 227 kJ. In designing a sulfuric acid plant, is it necessary to provide for heating or cooling of the reaction mixture? Explain.

Determine whether the statements given below are true or false. Consider an endothermic process taking place in a beaker at room temperature. (a) Heat flows from the surroundings to the system. (b) The beaker is cold to the touch. (c) The pressure of the system decreases. (d) The value of q for the system is positive.