Question

For substance A, the entropy of the solid at 98.36 K is 7.36 Cal/molK, at this...

For substance A, the entropy of the solid at 98.36 K is 7.36 Cal/molK, at this temperature it takes place the transition from one solid form to another, the transition heat is 284.3 cal/mol. The increase in entropy of the second solid modification is 98.36 K to 158.91 K and is 5.05 Cal/molK; The temperature of 158.91 K is the melting temperature of the solid. The melting heat of the solid is 476 cal/mol. From the melting point to the boiling point, 188.07 K, the increase of entropy is 2.36 Cal/molK and the heat of vaporization is 3860 cal/mol. A heat capacity from the boiling point to 298 K is 6.98 Cal/molK to an atmosphere of pressure. To calculate the absolute entropy of a considering as ideal gas an atmosphere and 298 K.

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Trouton’s rule states that the entropy of boiling at the normal point is 85 J/mol *...
Trouton’s rule states that the entropy of boiling at the normal point is 85 J/mol * K. (a) Does the data from Example 3.2 support Trouton’s rule? (b) H2O has a heat of vaporization of 40.7 kJ/mol. Does the Delta vapS for H2O at its normal boiling point support Trouton’s rule? Can you explain any deviation? (c) Predict the boiling point of cyclohexane, C6H12, if its Delta vapH is 30.1 kJ/mol. Compare your answer to the measured normal boiling point...
Determine the increase in entropy of solid magnesium when the temperature is increased from 300K to...
Determine the increase in entropy of solid magnesium when the temperature is increased from 300K to 800K at atmospheric pressure. The heat capacity is given by the following relation: Cp = 26.04 + 5.586 * 10^(-3)T + 28.476 * 10(4)T^(-2). Where Cp is in J/mol K, and?S =  ?Cp (dT/T)
Consider a pure crystalline solid that is heated from absolute zero to a temperature above the...
Consider a pure crystalline solid that is heated from absolute zero to a temperature above the boiling point of the liquid. Which of the following processes produces the greatest increase in the entropy of the substance? a. melting the solid b. heating the liquid c. heating the gas d. heating the solid e. vaporizing the liquid
A substance has the following properties: Heat capacities: 1.34 J/g oC (solid) 3.02 J/g oC (liquid)...
A substance has the following properties: Heat capacities: 1.34 J/g oC (solid) 3.02 J/g oC (liquid) 2.55 J/g oC (gas) Heat of Fusion = 4.23 kJ/mole Heat of Vaporization = 23.5 kJ/mole Melting Point = -30.0 oC Boiling Point = 88.5 oC Molar Mass = 69.3 g/mole How much energy (in kJ) would be needed to heat 555 g of this substance from 1 to 201oC?
A substance has a melting point of 20°C and a heat of fusion of 2.6×104 J/kg....
A substance has a melting point of 20°C and a heat of fusion of 2.6×104 J/kg. The boiling point is 150°C and the heat of vaporization is 5.2×104 J/kg at a pressure of 1.0 atm. The specific heats for the solid, liquid, and gaseous phases are 600 J/(kg·K), 1000 J/(kg·K), and 400 J/(kg·K), respectively. The quantity of heat required to raise the temperature of 3.0 kg of the substance from 3°C to 118°C, at a pressure of 1.0 atm, is...
A 500 g chunk of solid mercury at its 234 K melting point is added to...
A 500 g chunk of solid mercury at its 234 K melting point is added to 1500 g of liquid mercury at room temp (293 K). Determine the equilibrium mix and temperature. How much power does it take to raise the temperature of a 1.3 kg copper pipe by 15 oC/s? Relate this to the time you spend waiting for your shower to warm up. One inch copper pipe is .837 lb/foot. Assume that your shower is 30 feet from...
Heat is the Total internal energy of an object Average kinetic energy of molecules Measure of...
Heat is the Total internal energy of an object Average kinetic energy of molecules Measure of potential energy of molecules Same thing as very high temperature The specific heat of copper is 0.093 cal/g⁰C, and the specific heat of aluminum is 0.22  cal/g⁰C. The same amount of energy applied to equal masses, say, 50 g of copper and aluminum, will result in A higher temperature for copper A higher temperature for aluminum The same temperature for each metal Unknown results The...
Can you please check my answers and tell me if they are correct? thanks 8. Write...
Can you please check my answers and tell me if they are correct? thanks 8. Write the ionic equation for dissolution and the solubility product (Ksp) expression for each of the following slightly soluble ionic compounds: (a) PbCl2       PbCl2(s) --> Pb2+(aq) + 2Cl-(aq)                           Ksp = [Pb2+][Cl-]2   (b) Ag2S        Ag2S(s) --> 2Ag+(aq) + S2-(aq)                             Ksp =[Ag+]2[S2-] (c) Sr3(PO4)2 Sr3(PO4)2(s) --> 3Sr2+(aq) + 2PO43-(aq)         Ksp =[Sr2+]3[PO43-]2 (d) SrSO4       SrSO4(s) --> Sr2+(aq) + SO42-(aq)                       Ksp =[Sr2+][SO42-] 14. Assuming that no equilibria other than dissolution are involved,...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT