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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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
Transcribed Image Text:For antimony, Sb, the heat of fusion at its normal melting point of 631 °C is 19.6 kJ/mol.
The entropy change when 2.36 moles of solid Sb melts at 631 °C, 1 atm is
1
J/K.
FER
7
MacBook Pro
Expert Solution
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Question is based on the concept of chemical thermodynamics.
enthalpy of fusion is defined as the amount of heat required to change one mole of solid substance into liquid. entropy of fusion can be calculated by dividing enthalpy with melting point and multiplying with moles of the substance.
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- A certain substance has an enthalpy of fusion of 6.12 kJ/mol and an entropy of fusion of 22.3 J/mol/K. Calculate the approximate melting point of the substance. Leave the answer in Kelvin.arrow_forwardOxygen (O₂) is necessary for cellular respiration; it must be transported from the lungs to tissues through the bloodstream. However, O₂ is not very soluble in water. The Keq of oxygen dissolving at 300.0 K is 7.64 x 10⁻⁴ and the Keq at 320.0 K is 5.23 x 10⁻⁴. Calculate the ∆H(dissolve) for oxygen solubility in water, in kJ/mol.arrow_forwardFor silicon, Si, the heat of fusion at its normal melting point of 1410 °C is 46.4 kJ/mol. The entropy change when 2.12 moles of liquid Si freezes at 1410 °C, 1 atm is J/K.arrow_forward
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