Jibananda Paul and Subrata Kumar Choudhury Solutions for Chapter: Chemical Calculations, Exercise 1: EXERCISE

From the given equation $3\mathrm{Cu}+8{\mathrm{HNO}}_3\to \mathrm{Cu}{\left({\mathrm{NO}}_3\right)}_2+2\mathrm{NO}+4{\mathrm{H}}_2\mathrm{O}$, calculate the mass of copper required to react with $6.3 \mathrm{g} {\mathrm{HNO}}_3$.

Empirical formula of benzene is $\left(\mathrm{CH}\right)$. Vapour density of benzene is $39$. What is the molecular formula of benzene?

Determine the percentage of oxygen in ammonium nitrate.

When $100 \mathrm{g}$ of impure limestone is heated, the amount of residue left is $50.4 \mathrm{g}$. Calculate the percentage of purity of limestone.

$28 \mathrm{mL}$ sulphuric acid when reacts with $6.5 \mathrm{g}$ zinc $2.24 \mathrm{L}$ hydrogen gas at STP is obtained. Calculate the percentage of sulphuric acid. $\left[\mathrm{Zn} = 65 \mathrm{u}\right]$

Commercial zinc is only $65 \%$ pure. $50 \mathrm{g}$ of this commercial zinc is reacted with excess dilute sulphuric acid. Calculate the volume of ${\mathrm{H}}_2$ gas evolved at STP. $\left[\mathrm{Zn} = 65 \mathrm{u}\right]$

$2 \mathrm{g}$ Magnesium is heated with $2 \mathrm{g}$ sulphur. Calculate the amount of magnesium sulphide produced. Calculate the mass of the element that will be left as excess. $\left[\mathrm{Mg}=24 \mathrm{u}, \mathrm{S}=32 \mathrm{u}\right]$

Calculate the mass of carbon dioxide obtained from $10 \mathrm{kg}$ impure limestone. The sample of limestone is $90 \%$ pure. $\left[\mathrm{Ca} = 40 \mathrm{u}\right]$