a. Calculate the theoretical heat of reaction between the Zn and copper sulphate using the following enthalpy of formations:Formula is: ΔH0rxn = ∑nΔH0f (products) - ∑n (reactants)Zn(s) – (0 kJ/mol)ZnSO4 (aq) - (-152.4kJ/mol)Cu(s) – (0 kJ/mol)CuSO4 (aq) – (64.77 kJ/mol) b. In an experiment, 2 grams of zinc and 150 mL aq CuSO4 were made to react, then as observed, the temperature rises from 300C to 410C. What is the heat of the reaction between the zinc and copper sulphate (in kJ/mole)? Is the value near the theoretical value (found in item a)? Calculate the % error.% error = theoretical value-experimental value x 100Theoretical value

For question A, we use the given formula to calculate the theoretical heat of reaction.

Answered: a. Calculate the theoretical heat of…

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter2: Analyzing Data

Section2.3: Uncertainty In Data

Problem 48SSC

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Question

a. Calculate the theoretical heat of reaction between the Zn and copper sulphate using the following enthalpy of formations:

Formula is: ΔH⁰_rxn = ∑nΔH⁰_f(products) - ∑n (reactants)

Zn_(s) – (0 kJ/mol)

ZnSO₄ _(aq) - (-152.4kJ/mol)

Cu_(s)– (0 kJ/mol)

CuSO₄ _(aq) – (64.77 kJ/mol)

b. In an experiment, 2 grams of zinc and 150 mL aq CuSO₄ were made to react, then as observed, the temperature rises from 30⁰C to 41⁰C. What is the heat of the reaction between the zinc and copper sulphate (in kJ/mole)? Is the value near the theoretical value (found in item a)?