Standard Enthalpy Of Formation, Combustion And Bond Dissociation - Practice Questions & MCQ

A sample of ice at  is heated until it completely vaporizes into steam at .Calculate the total heat transfer during this process, including the heat required for fusion and vaporization. Additionally, determine the change in entropy during each phase transition and the total change in entropy for the entire process. Given the specific heat capacity of ice is , the specific heat capacity of water is , the heat of fusion of ice is ,  the heat of vaporization of water is , and the molar gas constant is .

Combustion of glucose $\left({\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6\right)$ produces ${\mathrm{CO}}_2$ and water. The amount of oxygen (in g) required for the complete combustion of $900\mathrm{g}$ of glucose is: $[$ Molar mass of glucose in $\mathrm{g}{\mathrm{mol}}^{-1}=180]$

The heat of combustion of ethanol determined by a bomb calorimeter is -670.48 Kcal/mol at 25°C. What is $\mathrm{\Delta }U$ at 25°C for the following reaction?

${\mathrm{C}}_2{\mathrm{H}}_5\mathrm{OH}(\mathrm{l})+\frac{7}{2}{\mathrm{O}}_2(\mathrm{g})\to 2{\mathrm{CO}}_2(\mathrm{g})+3{\mathrm{H}}_2\mathrm{O}(\mathrm{g})$

The standard enthalpy of formation (_fH^o₂₉₈) for methane, CH₄ is -74.9 kJ mol^-1. In order to calculate the average energy given out in the formation of a C - H bond from this it is necessary to know which one of the following?

Which one of the following orders is correct for the bond dissociation enthalpy of halogen molecules?

The bond dissociation energy is highest for

The correct order of bond enthalpy $\left({\mathrm{kJmol}}^{-1}\right)$ is :

Calculate the change in enthalpy when of water at is converted to steam at The heat of

vaporization of water is

Calculate the change in entropy $(\mathrm{\Delta }S)$ when 100 g of liquid water at ${100}^{\circ }\mathrm{C}$ is converted into steam at ${100}^{\circ }\mathrm{C}$. Given the heat of vaporization $\left(\mathrm{\Delta }{\mathrm{H}}_{\text{vap }}\right)$ of water is $40.79\mathrm{kJ}/\mathrm{mol}$.

A sample of ice at is heated until it becomes steam at .Calculate the total heat required to first raise the temperature of the ice to its melting point and then convert it to steam. Given the specific heat capacity of ice is , the heat of fusion of ice is ,the specific heat capacity of water is ,and the heat of vaporization of water is .