Calorimetry

If 3.365 g of ethanol ($l$) is burnt completely in a bomb calorimeter at 298.15 K, the heat produced is 99.472 kJ. The $|\Delta H_f^\circ|$ of ethanol at 298.15 K is ________ $\times10^2$ kJ mol$^{-1}$. (Nearest integer)
Given: Standard enthalpy for combustion of graphite = −393.5 kJ mol$^{-1}$
Standard enthalpy of formation of water (l) = −285.8 kJ mol$^{-1}$
Molar mass in g mol$^{-1}$ of C, H, O are 12, 1 and 16 respectively

The correct order of molar heat capacities measured at 298 K and 1 bar is :

2 mol of Hg($g$) is combusted in a fixed volume bomb calorimeter with excess of $\ce{O2}$ at 298 K and 1 atm into HgO($s$). During the reaction, temperature increases from 298.0 K to 312.8 K. If heat capacity of the bomb calorimeter and enthalpy of formation of Hg($g$) are 20.00 kJ K$^{-1}$ and 61.32 kJ mol$^{-1}$ at 298 K, respectively, the calculated standard molar enthalpy of formation of HgO($s$) at 298 K is X kJ mol$^{-1}$. The value of $|\mathrm X|$ is _____.

[Given: Gas constant $R = 8.3\ \mathrm{J\,K^{-1}\,mol^{-1}}$]

For complete combustion of methanol
$$\mathrm{CH_3OH(l)+\tfrac32O_2(g)\rightarrow CO_2(g)+2H_2O(l)}$$
the amount of heat produced as measured by bomb calorimeter is 726 kJ mol$^{-1}$ at 27°C. The enthalpy of combustion for the reaction is $-x$ kJ mol$^{-1}$, where $x$ is ______. (Nearest integer)

(Given : $R=8.3$ J K$^{-1}$ mol$^{-1}$)

2.4 g coal is burnt in a bomb calorimeter in excess of oxygen at 298 K and 1 atm pressure. The temperature of the calorimeter rises from 298 K to 300 K. The enthalpy change during the combustion of coal is $-x$ kJ mol$^{-1}$. The value of $x$ is ______. (Nearest Integer)

(Given : Heat capacity of bomb calorimeter 20.0 kJ K$^{-1}$. Assume coal to be pure carbon)

A gas (Molar mass = 280 g mol$^{-1}$) was burnt in excess $\mathrm{O_2}$ in a constant volume calorimeter and during combustion the temperature of calorimeter increased from 298.0 K to 298.45 K. If the heat capacity of calorimeter is 2.5 kJ K$^{-1}$ and enthalpy of combustion of gas is 9 kJ mol$^{-1}$ then amount of gas burnt is ______ g. (Nearest Integer)

When 600 mL of 0.2 M HNO$_3$ is mixed with 400 mL of 0.1 M NaOH solution in a flask, the rise in temperature of the flask is _______ $\times10^{-2}$ °C.

(Enthalpy of neutralisation = 57 kJ mol$^{-1}$ and Specific heat of water = 4.2 J K$^{-1}$ g$^{-1}$)

(Neglect heat capacity of flask)

A reversible cyclic process for an ideal gas is shown below. Here, $P$, $V$, and $T$ are pressure, volume and temperature, respectively. The thermodynamic parameters $q$, $w$, $H$ and $U$ are heat, work, enthalpy and internal energy, respectively.

The correct option(s) is (are)

The enthalpy change on freezing of 1 mol of water at 5°C to ice at −5°C is :

(Given $\Delta_{fus}H=6$ kJ mol$^{-1}$ at 0°C, $C_p(\ce{H2O}, l)=75.3$ J mol$^{-1}$ K$^{-1}$, $C_p(\ce{H2O}, s)=36.8$ J mol$^{-1}$ K$^{-1}$)

Enthalpy of dissociation (in kJ mol⁻¹) of acetic acid obtained from the Expt. 2 is

For complete combustion of ethanol,
$$\ce{C2H5OH(l) + 3O2(g) -> 2CO2(g) + 3H2O(l)},$$
the amount of heat produced as measured in bomb calorimeter, is 1364.47 kJ mol$^{-1}$ at 25°C. Assuming ideality the Enthalpy of combustion, $\Delta_cH$, for the reaction will be :

($R=8.314$ kJ mol$^{-1}$)

In a constant volume 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 298.0 K to 298.45 K due to the combustion process. Given that the heat capacity of the calorimeter is 2.5 kJ K$^{-1}$, the numerical value for the enthalpy of combustion of the gas in kJ mol$^{-1}$ is