Measurement of ΔU and ΔH using Calorimetry.

Four grams of graphite is burnt in a bomb calorimeter of heat capacity $30 \mathrm{kJ}/\mathrm{K}$ in excess of oxygen at 1 atmospheric pressure. The temperature rises from $300 \mathrm{to} 304 \mathrm{K}$. What is the enthalpy of combustion of graphite $(\mathrm{in} \mathrm{kJ} {\mathrm{mol}}^{-1})$?

Heat of combustion of ethanol at constant pressure and at temperature T K (= 298 K) is found to be $- \mathrm{q} \mathrm{J} {\mathrm{mol}}^{-1}.$ Hence, heat of combustion $(\mathrm{in} \mathrm{J} {\mathrm{mol}}^{-1})$ of ethanol at the same temperature at constant volume will be:

Calculate the ${\mathrm{\Delta H}}_{300\mathrm{K}}$ for the reaction ${\mathrm{NH}}_2{\mathrm{CN}}_{\left(\mathrm{s}\right)}+\frac{3}{2}{\mathrm{O}}_{2\left(\mathrm{g}\right)}\to {\mathrm{N}}_{2\left(\mathrm{g}\right)}+{\mathrm{CO}}_{2\left(\mathrm{g}\right)}+{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)}$ was carried out in a bomb calorimeter. The heat released was $743 \mathrm{kJ}{ \mathrm{mol}}^{-1}$.
[Given $\mathrm{R}=8.314 \mathrm{J}/\mathrm{Kmol}$]

Which of the following law is indicated by the principle of calorimeter?

State the principle of calorimeter.

The combustion of benzene (Molar mass $=78$ ) at ${27}^{\mathrm{o}}\mathrm{C}$ was found by bomb calorimeter for the reaction,

${\mathrm{C}}_6{\mathrm{H}}_6\left(\mathrm{l}\right)+7.5{\mathrm{O}}_2\left(\mathrm{g}\right)⟶6{\mathrm{CO}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)}$ 

to be $-3264 {\mathrm{kJmol}}^{-1}.$ Calculate the heat evolved on burning $39 \mathrm{g}$ of ${\mathrm{C}}_6{\mathrm{H}}_6$ in an open vessel (at $1$ atmospheric pressure).

In a constant pressure calorimeter, 3.5 g of a gas with molecular weight 28 was burnt in excess oxygen at 298.0 K. The temperature of the calorimeter was found to increase from 298 K to 298.45 K due to the combustion process. Given that the heat capacity of the calorimeter is 2.5 kJ ${\mathrm{K}}^{-1}$ , the value for the enthalpy of combustion of the gas is

When one mole of zinc dust and one mole of sulphuric acid react in a bomb calorimeter, then $\mathrm{\Delta }\mathrm{U}$ and $\mathrm{w}$ correspond to

When one mole of sulphuric acid react with one mole of zinc dust in a bomb calorimeter, then $\mathrm{\Delta }\mathrm{U}$ and $\mathrm{w}$ correspond to

At constant volume, 4 mol of an ideal gas when heated from 300 K to 500 K changes its internal energy by 5000 J. The molar heat capacity at constant volume is?

When the following reaction was carried out in a bomb calorimeter, $\mathrm{\Delta }\mathrm{U}$ is found to be $-\text{740}\text{.0}\text{kJ/mol}$ of ${\text{NH}}_{\text{2}}\text{CN(s)}$ (s) at $\text{300}\text{K}$.
$\mathrm{N}{\mathrm{H}}_2\mathrm{C}{\mathrm{N}}_{\left(\mathrm{s}\right)}+\mathrm{ }\frac{3}{2}{\mathrm{O}}_{2\left(\mathrm{g}\right)}\to {\mathrm{N}}_{2\left(\mathrm{g}\right)}+\mathrm{ }\mathrm{C}{\mathrm{O}}_{2\left(\mathrm{g}\right)}+\mathrm{ }{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)}$
Calculate ${\text{ΔH}}_{\text{300}\text{K}}$ for the reaction.

One mole of a non-ideal gas undergoes a change of state from $\text{(2}\text{.0}\text{atm,}\text{3}\text{.0}\text{L,}\text{100}\text{K)}$ to $\text{(4}\text{.0}\text{atm,}\text{5}\text{.0}\text{L,}\text{250}\text{K)}$ with a change in internal energy, $\mathrm{\Delta U}\hspace{0.33em}=\mathrm{\hspace{0.33em}}30.0\mathrm{\hspace{0.33em}}\mathrm{L} \mathrm{atm}$. The change in enthalpy of process (in L atm) is

What happens when we do not stir the mixture continuously in the experiment to determine the specific heat capacity of a given solid?

It takes 20 minutes to melt 10g of ice, when ray from the sun are focused by a lens of diameter 5 cm on to a block of ice. Calculate the heat received from the sun on $1\mathrm{ }\mathrm{c}{\mathrm{m}}^2$ per minute

(Given: L = 80 k cal/kg)

Water at $-{10}^{\mathrm{o}}\mathrm{C}$ is present in a thermally insulated container. Calculate the ratio of mass of ice formed and initial mass of water, if a small crystal of ice is thrown into it

The heat of reaction measured in a bomb calorimeter is:

The heat of reaction measured in a bomb calorimeter is:

The heat of reaction measured in a bomb calorimeter is:

The reaction of cyanamide ${\mathrm{N}\mathrm{H}}_2\mathrm{C}\mathrm{N}\mathrm{ }\left(\mathrm{s}\right)$ with oxygen was carried out in a bomb

caloriemeter and $\mathrm{\Delta }\mathrm{q}\mathrm{v}$ at $300\mathrm{ }\mathrm{K}$ was measured to be $-\mathrm{ }750\mathrm{ }\mathrm{k}\mathrm{J}/\mathrm{m}\mathrm{o}\mathrm{l}$. The value of $\mathrm{\Delta }\mathrm{H}$ per mole of ${\mathrm{N}\mathrm{H}}_2\mathrm{C}\mathrm{N}\mathrm{ }\left(\mathrm{s}\right)$ in the given reaction is-

In a calorimeter, the temperature of the calorimeter increases by 6.12 K, the heat capacity of the system is 1.23 kJ/g deg. What is the molar heat of decomposition for $\mathrm{N}{\mathrm{H}}_4\mathrm{N}{\mathrm{O}}_3?$