Answer to Question #196229 in General Chemistry for Benjamin

Question

5.0g of solid zinc carbonate are heated to produce oxide and carbon dioxide. 

(a) Write a balanced chemical equation for the reaction. States are required.

(b) Calculate the mass of carbon dioxide produced in the reaction.

Answer 1

(a) when zinc carbonate, ZnCO₃ decomposed, it formed solid zinc oxide, ZnO

 and carbon dioxide gas, CO₂

is released. So, balanced chemical equation is as follow: 

ZnCO_3(s)$\to$ ZnO_(S) +CO_2(g)

(b)It is given that mass of solid ZnCO₃

 is equal to 5.0 g

, and molar mass of ZnCO₃ is equal to 125.4 g/mol

. Put value of mass and molar mass of ZnCO₃ in the formula of number of moles and calculate number of moles of ZnCO₃

$N.o. of moles=\frac{5.0g}{125.4g/mol}$

$=0.04mol$

It is calculated that 0.04 moles of CO₂ are formed in the reaction. Calculate mass of CO₂  by putting value of number of moles and molar mass of CO₂ in the formula of number of moles. Molar mass of CO₂  is 44.01 g/mol.

$0.04mol=\frac{Given Mass }{44.01g/mol}$

Given Mass=0.04mol×44.01g/mol

=1.76g

So, 1.76 g of CO₂ is formed during the given chemical reaction.