1) A 45.9g sample of metal is heated to 95.5 Degrees Celsius and then placed in

Question

1) A 45.9g sample of metal is heated to 95.5 Degrees Celsius and then placed in a calorimeter containing 120.0 g of water (c=4.18 J/g`C) at 21.6 degrees celcius. The final temperature of water is 24.5 degrees celcius. Which metal was used?

I know the answer is Iron (c=0.45 J/g`C) but how do I get there?

2) The delta H value for a reaction is -90.8 kJ. How much heat is released when 63.8 g Hg is reacted with oxygen?

3) A chunk of iron at 90.6 degrees celcius was added to 200.0 g of water at 15.5 deg C. The specific heat of iron is 0.449 J/g`C, and the specific heat of water is 4.18 J/g`C. When the temperature stabilized, the temperature of the mixture was 18.2 deg C. Assuming no heat was lost to the surroundings, what was the mass of iron added?

4) Give all the possible values of l for a 3 sublevel

5) identify the correct values for a 1s sublevel

a) n=3, l=1, ml=0

b) n=2, l=1, ml= -2

c) n=1, l=0, ml=0

d) n=2, l=0, ml=0

e) n=4, l= -1, ml= -2

Please explain the answers as much as possible! Thank you!

Explanation / Answer

heat lost by metal = heat gained by water

specific heat of metal x mass x temp change = specific heat of water x mass x temp change

S x 45.9 x ( 95.5-24.5) = 4.18 x 120 x ( 24.5-21.6)

S = 0.446 J/gmK   = 0.45 J/gmK

3) heat lost by metal = heat gained by water

0.449(90.6-18.2) x mass of meatl = 200x(18.2-15.5) x4.18

mass of metal = 69.44 gm

5) c is answer

1s n= 1 , and

for s we have l = 0 ,

and m l can have values of +l to -l and hence ml = 0

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