$20 \ g$ of hydrogen gas $(H_2)$ is present in a $5 \ L$ vessel. The molar concentration of hydrogen is: (in $M$)

$P_4O_6$ reacts with water according to the equation $P_4O_6 + 6H_2O \to 4H_3PO_3$. Calculate the volume of $0.1 \ M$ $NaOH$ solution required to neutralize the acid formed by dissolving $1.1 \ g$ of $P_4O_6$ in $H_2O$. (in $mL$)

The exact volumes of $1\, M\, NaOH$ solution required to neutralize $50\, mL$ of $1\, M\, H_3PO_3$ solution and $100\, mL$ of $2\, M\, H_3PO_2$ solution,respectively,are:

$56.0 \ L$ of nitrogen gas is mixed with excess of hydrogen gas and it is found that $20 \ L$ of ammonia gas is produced. The volume of unused nitrogen gas is found to be $L$.

The volume of $0.02 \, M$ aqueous $HBr$ required to neutralize $10.0 \, mL$ of $0.01 \, M$ aqueous $Ba(OH)_2$ is $....... \, mL$ (Assume complete neutralization).

How many moles of $H_2O$ (per mole of $Cl_2$ evolved) will be formed when $KMnO_4$ is added to $HCl$ solution?