$A$ bottle of cold drink contains $200 \ mL$ liquid in which $CO_2$ is $0.1 \ M$. Suppose $CO_2$ behaves like an ideal gas,the volume of the dissolved $CO_2$ at $STP$ is (in $L$)

What volume of $CO_2$ at $STP$ is obtained by thermal decomposition of $20 \ g$ $KHCO_3$? [Atomic weight of $K = 39$]
$2KHCO_{3(s)} \to K_2CO_{3(s)} + CO_{2(g)} + H_2O_{(g)}$

The heat of combustion of methane is $-800 \ kJ \ mol^{-1}$. What is the heat of combustion for $4 \times 10^{-4} \ kg$ of methane?

When $1 \ dm^{3}$ of $CO_{2}$ gas is passed over hot coke, the volume of the gaseous mixture after the complete reaction at $STP$ becomes $1.4 \ dm^{3}$. The composition of the gaseous mixture at $STP$ is:

The heat of combustion of methane is given by the following equation. How many grams of methane are required to produce $445 \ kJ$ of heat (in $g$)?
$CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O \ (\Delta H = -891 \ kJ/mol)$

One mole of calcium phosphide on reaction with excess of water gives