The molar heat capacity, C_m of gold (Fe(s)) is 25.1 J K^-1 mol^-1. Calculate the energy (in J) required to heat a 25 g bar of iron from 50 °C to 75 °C.

The specific heat capacity of liquid water is 4.18 J K^-1 g^-1. Calculate the temperature rise (in K) when 350 J of heat is transferred to 3 mol of water.

The specific heat capacity of iron (Fe(s)) is 0.38 J K^-1 g^-1, how much energy (in J) must be added to raise the temperature of a 100 g copper bar by 25 °C?

The standard enthalpy change of vaporization of ethanol is + 43.5 kJ mol^-1. Calculate the enthalpy change (in kJ) when 23 g of ethanol vaporizes at its boiling point at 1 bar.

Calculate the standard enthalpy change (in kJ mol^-1) for the hydrogenation of pentene to pentane at 298 K. The standard enthalpy change at 298 K for reactions of graphite and hydrogen gas to form 1 mol of each of these compounds is −21.7 kJ mol^-1 and −146.8 kJ mol^-1 respectively.

Calculate for the oxidation of 2-propanol to propanone:

C₃H₇OH (g)+ ½ O₂ (g)→ C₃H₆O (g) + H₂O (g)

using the bond enthalpies given in Table 13.5

The enthalpy change for a reaction at 298 K is –35.5 kJ mol^-1.

Calculate the enthalpy change at 333 K if the difference in heat capacities between reactants and products, DC_Pis 14.4 J mol⁻¹ K⁻¹.

A reaction produces carbon dioxide gas. A balloon attached to the reaction vessel expands against a constant pressure of 1.1 atm and at the end of the reaction it is calculated that 2.5 dm³ of CO₂ (g) has been produced. Calculate the energy transferred as work, w, (in J).

One mole of gas is heated with 4.2 kJ of energy; it expands doing 3250 J of work. Calculate the change in internal energy of the gas.

The combustion of benzoic acid at 1 bar and 298 K releases 3228 kJ mol^-1 of heat.

C₇H₆O (s) + 8 O₂ (g) → 7 CO₂ (g) + 3 H₂O (l) Calculate (in kJ mol^-1) for benzoic acid.