When energy is added to a liquid, its particles begin to move (kinetic energy increases). If sufficient energy is the particles will completely the intermolecular forces, which causes them to move from each other. When this happens, the liquid ; When energy is removed from a gas, the particles begging to; Since the particles are moving the pull of intermolecular forces on them gets If sufficient energy is the intermolecular forces can pull them together, allowing them to only move each other. Then, the gas: 620 DAA O Type here to search

Consider the Sublimation of dry ice (solid carbon dioxide). The value of deltaHsub for CO2 is 25.2kj/mol  1) write the balanced chemical equation for the sublimation of CO2 2) Is this reaction "breaking bonds" (intramolecular) or "breaking intermolecular forces" (intermolecular)? What's the difference between the two?

Unit Name: Thermodynamic Chemistry When there is going to be a frost in Florida, farmers will spray their crops with water before the frost hits thereby preventing the fruit from freezing. Using concepts from this unit, explain why this helps to save the fruit

Ice at -4.80oC is added to 220g of water at 26.60oC. What is the mass of ice needed to cool the water to an equilibrium temperature of 22.2oC?

Which change does heat energy cause? greater energy differences between molecules reduced energy transfer more collisions between molecules slower molecule movement

Consider the following phase change equilibrium: CHCl3(s)= CHCl3(l) If delta H* is 9.74 kJ/mol and delta S* is 40.00 J/mol K, determine the melting point of CHCl3 in K?

What is the total enthalpy change during the process in which 100.0 g of water at 50.0 °C is cooled to ice at -30.0 °C ? (Assume P = 1.0 atm). Note: COOLING is an EXOTHERMIC PROCESS!!! AH WILL BE NEGATIVE! Solution S.H. water = 4.18 J/g °C Temperature AHfus = 6.01 kJ/mol 50.0 °C 0.0 °C 1 -30.0 °C 2 3 S.H. ice = 2.03 J/g °C 100.0 g H₂O = 5.552 mol H₂O 18.01 g/mol ΔΗ, = SH x Υ x ΔΤ AH₁ = (4.18 J/g °C)(100.0 g)(0.0 - 50.0 °C) == - 20900 J - 20.9 kJ Energy (J) Thus the total enthalpy change is: AH₂ = -AHfus XY AH₂ = -(6.01 kJ/mol)(5.552 mol) = -33.4 kJ ΔΗ, = SH x Υ x ΔΤ AH3 = (2.03 J/g °C)(100.0 g)(- 30.0 - 0.00 °C) = 6090 J = - 6.09 kJ -20.9 kJ-33.4 kJ - 6.09 kJ = - 60.4 kJ

How do I read the structures... I'm confused

I need the answer to question 7

The heat of vaporization for ethanol is 0.826 kJ/g. Calculate the heat energy in joules required to boil 62.75g of ethanol heat energy: in joules