Generate the heating graph for H₂O. Determine the quantity of energy transfer required to heat 1.0 g solid H₂O from -50 °C to the melting point, 0 °C. X J

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Q: 5,6

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A: Wavelength of photon absorbed = 97.20 nm

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Q: what is the product produced when 2-methyl-3-bromohexane reacts with tert-butoxide

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Q: uggest an arrow pushing mechanism for the transformation below. OH NH₂ Pd(OAc)2 (cat.) air, MeOH

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Q: Which of the following chemical equations demonstrates the law of conservation of mass?

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Q: Molecular formula Empirical formula

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Q: MORE PRACTICE: Balance by oxidation Number Method. 1. MnO, + SO, Mn² + SO² ... in acid. -

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Q: Estimate the pH of 0.10 M H₂SO4, Ka1 large, Ka2 = .012

A: Detail

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.    

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.