How much energy in kJ is required to fully vaporize (at temperature of boiling point =...

How much energy in kJ is required to fully vaporize (at temperature of boiling point = 2525C) a 270g sample of Al(s), initially at 25C?

(Enthalpy of vap = 300. kJ/mol, enthalpy of fusion = 11. kJ/mol)

(specific heat of aluminum for both solid and liquid form = 0.9 J/(K * g))

(temperature of melting point = 625C, temp of boiling point = 2525C)

Solutions

Expert Solution

no of moles of Al = W/G.M.Wt

= 270/27 = 10moles

q1 = mCT

= 270*0.9*(625-25)

= 145800J = 145.800KJ

q2 = no of moles*enthalpy of fusion

=10*11 = 110Kj

q3 = mCT

= 270*0.9*(2525-625)

= 461700J = 461.7KJ

q4 = no of moles * Enthalpy of vap

= 10*300 = 3000KJ

Total energy = q1+q2+q3+q4

= 145.8+110+461.7+3000 = 3717.5KJ

queen_honey_blossom answered 10 months ago

Next > < Previous

Related Solutions

1. How much energy(kJ) is required to vaporize 10 kg of water at 500 kPa? 2....

1. How much energy(kJ) is required to vaporize 10 kg of water at 500 kPa? 2. What is the state of water of 150 deg Celcius and 415.7 kPa?

How much heat is required? The Melting point of H2O(s) is Oc, the boiling point of...

How much heat is required? The Melting point of H2O(s) is Oc, the boiling point of H2O (l) is 100c, and H2O has the following thermodynamic data: Cm(H2O(l)) = 75.4 J/mol*C deltHfus = 6.01 kJ/mol Cm(H2O(g)) = 33.6 J/mol*C deltHvap = 40.67 kJ/mol How much heat is required to convert 25.0g of H2O(s) at 0c to H2O(g) at 115c?

How much energy (in kJ) is required to convert a 2.56 lb block of ice at...

How much energy (in kJ) is required to convert a 2.56 lb block of ice at -12.5oF to steam at 234oF? Use the space provided on this page to draw a complete heating curve, labeling the axes and each important point on the graph. Below the graph, show your calculations and the final answer.

How much energy, in kiloJoules, would be required to raise the temperature of 1.00 kilogram of...

How much energy, in kiloJoules, would be required to raise the temperature of 1.00 kilogram of liquid benzene (C6H6) from 20.0 dC to its boling point of 80.1dC and then to completely vaporize the benzene at this same temperature? The specific heat capacity of benzene is 1.74J g-1 0C-1. The molar enthalpy of vaporization of benzene is 1.929 kJ/mole.

How much energy is required to raise the temperature of 100g of water from -10 to...

How much energy is required to raise the temperature of 100g of water from -10 to 110°C?

At 1 atm, how much energy in kJ is required to heat 85.0 g H 2...

At 1 atm, how much energy in kJ is required to heat 85.0 g H 2 O ( s ) at − 10.0 ∘ C to H 2 O ( g ) at 167.0 ∘ C? Use the heat transfer constants found in this table. Quantity per gram per mole Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H2O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) * Specific heat of liquid...

Calculate how much energy is required to heat 20 mL of water from room temperature to...

Calculate how much energy is required to heat 20 mL of water from room temperature to 40 C & also how much energy is released when 20 mL of water is cooled from the initial temperature to 10 C

Given a liter of water just at boiling, how much energy does it take to boil...

Given a liter of water just at boiling, how much energy does it take to boil it all?

a) The reaction temperature for this lab is significantly above the boiling point of the solvent...

a) The reaction temperature for this lab is significantly above the boiling point of the solvent used (ethanol boils at 78 o C; the reaction mixture was heated up to 140 o C). Why are we able to conduct reactions above the boiling point of the solvent when using our microwave oven in lab? b) Explain why hexane is a very poor choice as a solvent for a microwave reaction. c) After developing a TLC plate, a student looks at...

When external pressure decreases which occurs? 1) boiling point decreases 2) boiling point increases 3) temperature...

When external pressure decreases which occurs? 1) boiling point decreases 2) boiling point increases 3) temperature increases 4) liquid condense 5) none of these

Subjects