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ICSE Class 10 Chemistry Question 30 of 37

Mole Concept and Stoichiometry — Question 1

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Question 1

The reaction between 15 g of marble and nitric acid is given by the following equation:

CaCO3 + 2HNO3 ⟶ Ca(NO3)2+ H2O + CO2

Calculate:

(a) the mass of anhydrous calcium nitrate formed

(b) the volume of carbon dioxide evolved at S.T.P.

Answer

CaCO3+ 2HNO3⟶Ca(NO3)2+ H2O +CO240+12+3(16)40+2(14)+6(16)=40+12+4840+28+96=100 g164 g\begin{matrix} \text{CaCO}_3 & + \space 2\text{HNO}_3 \longrightarrow & \text{Ca(NO}_3)_2 & + \space \text{H}_2\text{O} \space + \text{CO}_2 \\ 40 + 12 + 3(16) & & 40 + 2(14) + 6(16) \\ = 40 + 12 + 48 & & 40 + 28 + 96 \\ = 100 \text{ g} & & 164 \text{ g} \end{matrix}

100 g of CaCO3 produces = 164 g of Ca(NO3)2

∴ 15 g CaCO3 will produce = 164100\dfrac{164}{100} x 15

= 24.6 g

Hence, mass of anhydrous calcium nitrate formed = 24.6 g

(b) 100 g of CaCO3 produces = 22.4 litres of carbon dioxide

∴ 15 g of CaCO3 will produce = 22.4100\dfrac{22.4}{100} x 15

= 3.36 litres of CO2