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How many kilojoules (to 3 s.f.) of energy is required to heat 90.0 g H₂O (5.00 moles) from solid ice at -16.0°C to a liquid at 81.0°C? The following physical data may be useful.

How many kilojoules (to 3 s.f.) of energy is required to heat 90.0 g H₂O (5.00 moles) from solid ice at -16.0°C to a liquid at 81.0°C? The following physical data may be useful.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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## Constants: - \( c = 2.9979 \times 10^8 \) m/s - \( h = 6.626 \times 10^{-34} \) J per one photon - \( R = 8.314 \) J/(K mol) = 0.08206 L atm/(K mol) - \( N_A = 6.022 \times 10^{23} \) particles/mol - \( R_H = 1.097 \times 10^7 \) m\(^{-1} = 2.178 \times 10^{-18} \) J --- ### Problem Statement: **Question:** How many kiloJoules (to 3 significant figures) of energy is required to heat 90.0 g H\(_2\)O (5.00 moles) from solid ice at \(-16.0^\circ\)C to a liquid at 81.0°C? The following physical data may be useful: - \( \Delta H_{\text{fus}} = 6.02 \) kJ/mol - \( \Delta H_{\text{vap}} = 40.7 \) kJ/mol - \( C_{\text{liq}} = 4.184 \) J/g°C - \( C_{\text{gas}} = 2.01 \) J/g°C - \( C_{\text{sol}} = 2.09 \) J/g°C - \( T_{\text{melting}} = 0^\circ\)C - \( T_{\text{boiling}} = 100^\circ\)C --- This content aims to assist students in understanding the amount of energy required to change the state and temperature of a given mass of water from ice at a subzero temperature to liquid at a specified elevated temperature. The constants provided are fundamental for many thermodynamic and quantum mechanics calculations, while the problem requires applying knowledge of thermodynamic equations and phase change enthalpies.
Transcribed Image Text:## Constants: - \( c = 2.9979 \times 10^8 \) m/s - \( h = 6.626 \times 10^{-34} \) J per one photon - \( R = 8.314 \) J/(K mol) = 0.08206 L atm/(K mol) - \( N_A = 6.022 \times 10^{23} \) particles/mol - \( R_H = 1.097 \times 10^7 \) m\(^{-1} = 2.178 \times 10^{-18} \) J --- ### Problem Statement: **Question:** How many kiloJoules (to 3 significant figures) of energy is required to heat 90.0 g H\(_2\)O (5.00 moles) from solid ice at \(-16.0^\circ\)C to a liquid at 81.0°C? The following physical data may be useful: - \( \Delta H_{\text{fus}} = 6.02 \) kJ/mol - \( \Delta H_{\text{vap}} = 40.7 \) kJ/mol - \( C_{\text{liq}} = 4.184 \) J/g°C - \( C_{\text{gas}} = 2.01 \) J/g°C - \( C_{\text{sol}} = 2.09 \) J/g°C - \( T_{\text{melting}} = 0^\circ\)C - \( T_{\text{boiling}} = 100^\circ\)C --- This content aims to assist students in understanding the amount of energy required to change the state and temperature of a given mass of water from ice at a subzero temperature to liquid at a specified elevated temperature. The constants provided are fundamental for many thermodynamic and quantum mechanics calculations, while the problem requires applying knowledge of thermodynamic equations and phase change enthalpies.
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