A metal M forms a volatile carbonyl complex $M(CO)_x$. 0.525g of this complex is heated in a closed vessel of volume 250 mL at $50^\circ C$. The pressure inside the vessel after complete decomposition of the complex is 746 Torr. If the gas constant R is 0.0821 L atm $K^{-1} mol^{-1}$, what is the value of x in the formula $M(CO)_x$? (Assume the metal M does not contribute significantly to the pressure)

100 mL of 0.1 M solution of a reductant is diluted to 1 litre, which of the following changes?

How many litre of ${\rm{C}}{{\rm{l}}_2}$ at STP will be liberated by the oxidation of ${\rm{NaCl}}$ with 10 g ${\rm{KMn}}{{\rm{O}}_4}$?

When one mole of ${\rm{KMn}}{{\rm{O}}_4}$ reacts with $HCl$, the volume of chlorine liberated at $NTP$ will be:

A solution is prepared by dissolving 10 g of glucose in 190 g of water. What is the mass percentage of glucose in the solution?

A solution is prepared by dissolving 10 g of sucrose ($C_{12}H_{22}O_{11}$) in 200 g of water. What is the mole fraction of sucrose?

For the reaction, $2{\rm{F}}{{\rm{e}}^{3 + }} + {\rm{S}}{{\rm{n}}^{2 + }} o 2{\rm{F}}{{\rm{e}}^{2 + }} + {\rm{S}}{{\rm{n}}^{4 + }}$ The normality of ${\rm{SnC}}{{\rm{l}}_2}$ (mol.wt. = 189.7) solution prepared by dissolving 47.5 g in acid solution and diluting with ${{\rm{H}}_2}{\rm{O}}$ to a total of 2.25 litre is :

0.5 grams of sodium hydroxide was treated with $12.5 \mathrm{mL}$ of $0.75 \mathrm{M}$ HCl solution. The mass of sodium hydroxide left unreacted is equal to

What is the mole fraction of the solute in a 1.00 m aqueous solution of glucose?

Weight of ${\rm{FeS}}{{\rm{O}}_4}\left( {{\rm{mol}}{\rm{.wt}}{\rm{.}} = 152} \right)$ oxidized by 200 mL of 1 $N$ ${\rm{KMn}}{{\rm{O}}_4}$ solution is :

What is the normality of a ${\rm{KMn}}{{\rm{O}}_4}$ solution to be used as an oxidant in acid medium, which contain 15.8 g of the compound in 100 mL of solution? Mol. wt. of ${\rm{KMn}}{{\rm{O}}_4}$ is 158 :