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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

You should use care when dissolving H2SO4 in water because the process is highly exothermic. To measure the enthalpy change, 5.2 g of concentrated H2SO4() was added (with stirring) to 135 g of water in a coffee-cup calorimeter. This resulted in an increase in temperature from 20.2 °C to 28.8 °C. Calculate the enthalpy change for the process H2SO4() → H2SO4(aq), in kf/mol.

Interpretation Introduction

Interpretation:

The enthalpy change for the reaction for dissolving H2SO4 in water has to be determined.

Concept Introduction:

Standard enthalpy of the reaction,ΔrHo is the change in enthalpy that happens when matter is transformed by a given chemical reaction, when all reactants and products are in their standard states.

Enthalpy of the reaction, ΔrH, is the change in enthalpy that happens when matter is transformed by a given chemical reaction

Heat energy required to raise the temperature of 1g of substance by 1K..Energy gained or lost can be calculated using the below equation.

  q=C×m×ΔT

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity,ΔT= change in temperature.

Explanation

Given,

  Specific heat capacity of the solution=4.20JK/g

  Mass of H2SO4=5.2g

  Mass of water =135g

Determine the amount of H2SO4

  5.2g(1mol÷98.079g) = 0.053mol

Assume qr+qsol=0

  qsol can be calculated from q=C×m×ΔT, as

  qsol= (5.2g of H2SO4 + 135g of water) × 4

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