What quantity of energy does it take to convert 1.29 kg of ice at-23 degree c to

Question

What quantity of energy does it take to convert 1.29 kg of ice at-23 degree c to water at 35 degree c? specific heat capacities: ice 2.03 J/log degree c) and liquid water 4.184 J/(g degree C) Delta H_vap = 40.7 kJ/mol; Delta H_vs = 6.02 kJ/mol 742 kJ 257 3.59 times 10^3 6.04 times 10^4 680 Use the diagram below to tell which of the following is NOT true. Melting occurs along the CB line. denser than the liquid. According to the diagram, the solid phase of this substance is denser than the liquid. From the phase diagram above, the minimum pressure at which this substance can exist in the liquid phase is 0.25 atm. The solid and liquid phases can exist in equilibrium along line CB. The temperature and pressure at which all three phases can coexist in equilibrium is 0.45 atm and 130 degree C. Which of the following is/are true? non-directional covalent bonds. Diamond is a network solid with high melting point and non-directional covalent bonds. Water is a molecular solid held together with hydrogen-bonds. dispersion forces. Brass is a metallic solid, a conductor, and is held together with London dispersion forces. Magnesium phosphate is an ionic solid, a conductor, and has a low melting point. All of these are true.

Explanation / Answer

9. Total energy needed

= 1.29 x 10^3 x 2.03 x 23/1000 + 1.29 x 10^3 x 6.02/18 + 1.29 x 10^3 x 4.184 x 35/1000

= 60.23 + 431.43 + 189.00

= 680.57 kJ

E) 680 kJ

10) From the diagram , false statements would be,

C)

11. True statements would be,

A) Diamond is a network solid with non-directional covalent bonds.

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