Answer to Question #196229 in General Chemistry for Benjamin

Question #196229

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.

Expert's answer

(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: 

ZnCO3(s)"\\to" ZnO(S) +CO2(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}"


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


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

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