A 1.200 g sample of ZnCO3 (s) dissolved in 40.0 mL of a dilute HCl solution (density = 1.10 g/mL) in a coffee cup calorimeter, producing CO2 (g), liquid water and ZnCl2 (aq).  The temperature of the solution changes from 24.32 oC to 25.49 oC.  The resulting solution has a specific heat of 4.18 J/goC.What would be the # of heat released by the reaction and Is the reaction endothermic?

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Asked Oct 25, 2019
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A 1.200 g sample of ZnCO3 (s) dissolved in 40.0 mL of a dilute HCl solution (density = 1.10 g/mL) in a coffee cup calorimeter, producing CO2 (g), liquid water and ZnCl2 (aq).  The temperature of the solution changes from 24.32 oC to 25.49 oC.  The resulting solution has a specific heat of 4.18 J/goC.

What would be the # of heat released by the reaction and Is the reaction endothermic?

 

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Expert Answer

Step 1

The required equation is given below.

ZnCO, (s)+ 2HC1(aq) - ZnCl, (aq) +H20(1I)+CO, (g)
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ZnCO, (s)+ 2HC1(aq) - ZnCl, (aq) +H20(1I)+CO, (g)

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Step 2

The heat of the reaction in a calorimeter can be calculated by using the given below formula.

AH2(m)s)(AT)
Where,
misthetotalmass of sample taken in the calorimeter
sis the specific heat capacity of the calorimeter
ATisthe changein temperaturein 'C
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AH2(m)s)(AT) Where, misthetotalmass of sample taken in the calorimeter sis the specific heat capacity of the calorimeter ATisthe changein temperaturein 'C

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Step 3

The heat of the given reaction in a calorime...

Totalmass of thesample =mass of ZnCO,
mass of HCl
gg
= (1.2g)+40.0 mL x 1.10 x -
mL
= 45.2g
Where,
mass
density
Volume
density of HClis1.10g /mL
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Totalmass of thesample =mass of ZnCO, mass of HCl gg = (1.2g)+40.0 mL x 1.10 x - mL = 45.2g Where, mass density Volume density of HClis1.10g /mL

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