The combustion reaction of glucose is given as: (Molar mass of glucose = $180 \ g/mol$) $C_6H_{12}O_6 + 6O_2 \rightarrow 6CO_2 + 6H_2O, \Delta H = -72 \ kcal$. The energy required for the production of $1.6 \ g$ of glucose is .......... $kcal$.

Equal masses in grams of $H_2$, $N_2$, $Cl_2$, and $O_2$ are enclosed in cylinders separately. If these gases expand isothermally and reversibly by $10 \ dm^3$ at $300 \ K$, the work done by the gas is maximum for:

$A$ pre-weighed vessel is filled with $O_2$ and weighed at $STP$. It is then evacuated and filled with $SO_2$ gas at the same temperature and pressure,and weighed again. The weight of $O_2$ will be:

In the petroleum industry,a process is carried out to increase the octane number of fuel as follows: $C_7H_{14} \rightarrow C_7H_8 + 3H_2$. In this process,two hydrocarbons are in liquid state while $H_2$ is in gaseous state. What is the percentage decrease in the weight of the liquid in the above reaction?

At $STP$,'$x$' $g$ of a metal hydrogen carbonate $(MHCO_3)$ (molar mass $84 \ g \ mol^{-1}$) on heating gives $CO_2$,which can completely react with $0.2 \ mol$ of $MOH$ (molar mass $40 \ g \ mol^{-1}$) to give $MHCO_3$. The value of '$x$' is

What volume of ammonia is formed when $10 \ dm^3$ dinitrogen reacts with $30 \ dm^3$ dihydrogen at same temperature and pressure (in $dm^3$)?