CHEM 1010H Chapter 6: CHEM 1010H Answers, 6.126

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22 Jan 2016

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Liquid water at a temperature t (the t in the question for your mastering chemistry assignment) You are trying to find h, u, q and w. Step 1 is going from liquid at t to liquid at 0 c. Step 3 is going from solid at 0 c to solid at t. At constant pressure remember that h = q. Step 2 is going from liquid at 0 c to solid at 0 c. Step 4 is going from liquid at t to solid at t. For steps 1 and 3 q = mcs t and the units will still contain the unit g) (except they do not give you m so leave it out of the equation. Assume that the density of the phase does not change (too much with temperature) at your given temperature. (so use the densities i listed above for the volume calculation). Volume is v solid v liquid work = w = -p v.

Related Questions

The triple point of water is at 273.16 K and 611.73Pa. Near the triple point, the enthalpy of vaporization of
H2O is 44.07 kJ/mol and the enthalpy of fusion is 6.008 kJ/mol (assume both are constant at all temperatures).The density of the solid ice is 0.917 g cm-3 and the density of the liquid is 0.9998 g cm-3 near the triple point.Assume the vapor behaves ideally.

Make a quantitative graph of the phase diagram of water (P vs T phase boundaries) in the vicinity of the triplepoint Do not make any approximations that the curves are linear for the liquid/gas or solid/gas boundaries Hint:to plot the near-vertical liquid/solid line on this scale, you will need to pick a very narrow range of temperaturesin your spreadsheet or graphing program. A range of -10 Celsius to +10 Celsius and 0 to 1600 Pa is suggested

Heat, q, is energy transferred between a system and its surroundings. For a process that involves a temperature change

q=mâ Csâ ÎT

where Cs is specific heat and m is mass.

Heat can also be transferred at a constant temperature when there is a change in state. For a process that involves a phase change

q=nâ ÎH

where, n is the number of moles and ÎH is the enthalpy of fusion, vaporization, or sublimation.

The following table provides the specific heat and enthalpy changes for water and ice.

Substance	Specific heat [J/(gâ âC)]	ÎH (kJ/mol)
water	4.18	44.0
ice	2.01	6.01

Part A

Calculate the enthalpy change, ÎH, for the process in which 45.7 g of water is converted from liquid at 10.1 âC to vapor at 25.0 âC .

For water, ÎHvap = 44.0 kJ/mol at 25.0 âC and Cs = 4.18 J/(gâ âC) for H2O(l).

Part B

How many grams of ice at -12.5 âC can be completely converted to liquid at 8.1 âC if the available heat for this process is 5.27Ã10³ kJ ?

For ice, use a specific heat of 2.01 J/(gâ âC) and ÎHfus=6.01kJ/mol.

Express your answer to three significant figures and include the appropriate units.

CHEM 1010H Chapter 6: CHEM 1010H Answers, 6.126

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