(a) Interpretation Introduction To determine: The change in enthalpy ( Δ H ) for the given process. Explanation Given The given mass of NH 4 NO 3 is 4.25 g . The given mass of water is 60.0 g . The total mass of sample is 64.25 g . The initial temperature is 22.0 ° C . The final temperature is 22.0 ° C . The change in temperature = 22 ° C − 16.9 ° C = 5 .1 ° C = 5 .1 K The specific heat of water is 4.184 J / g ⋅ ° C . The amount of heat transferred is calculated using the formula, q = − ( m × s × Δ T ) Where, q is the amount of heat transferred. m is the mass. s is the specific heat. Δ T is the change in temperature. Substitute the values of m , s and Δ T in the above expression, q = ( − ( 64.25 g ) × ( 4.184 J / g ⋅ ° C ) × ( 5.1 K ) ) = − 1370.9 J = − 1 .371 kJ At constant pressure, the heat transferred is equal to the change in enthalpy. Therefore, the change in enthalpy is − 1.371 kJ (b) Interpretation Introduction To determine: If the given process is exothermic or endothermic.

Chemistry: The Central Science (14th Edition)

14th Edition

ISBN: 9780134414232

Author: Theodore E. Brown, H. Eugene LeMay, Bruce E. Bursten, Catherine Murphy, Patrick Woodward, Matthew E. Stoltzfus

Publisher: PEARSON

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Chapter 5, Problem 56E

(a)

Interpretation Introduction

To determine: The change in enthalpy (ΔH) for the given process.

(b)

Interpretation Introduction

To determine: If the given process is exothermic or endothermic.

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Chapter 5, Problem 55E

Chapter 5, Problem 57E

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Chemistry: The Central Science (14th Edition)

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