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FinnZ [79.3K]
3 years ago
6

Calculate the amount of energy released when 2,064 g of water are cooled from 92 ˚C to 45˚C. The specific heat of water is 4.184

.
Chemistry
1 answer:
Andrews [41]3 years ago
8 0

Answer: Q= - 405,881 J or -405.88 kJ

Explanation: To find the amount of heat released we will use the formula of heat which is Q = mc∆T.

Q= 2,064 g ( 4.184 J/g°C) ( 45°C -92°C)

= 2,064 g ( 4.184 J/g°C) ( -47°C)

= -405,881 J

Or we can convert this into kJ which is equal to -405.88 kJ.

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state of matter

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3 0
3 years ago
When 15.3 g of sodium nitrate, NaNO3,was dissolved in water in a calorimeter, the temperature fell from 25.00oC to 21.56oC. If t
satela [25.4K]

Answer:

20.468 kilo Joules is the enthalpy change when one mole of sodium nitrate dissolves.

Explanation:

Heat lost by solution ad calorimeter = Q

Heat capacity of solution ad calorimeter = C = 1071 J/°C

Change in temperature = ΔT = 21.56°C - 25.00°C = -3.44°C

Q=C\times Delta T

Q=1071 J/^oC\times (-3.44^oC)=-3,684.24 J

Heat gained by sodium nitrate = -Q = -(-3,684.24 J)=3,684.24 J

Moles of sodium nitrate = \frac{15.3 g}{85 g/mol}=0.18 mol

When 0.18 mole of sodium nitrate was dissolved in water 3,684.24 joulesof heat was absorbed by it.

Then heat absorbed by 1 mole of sodium nitrate :

\frac{3,684.24 J}{0.18}=20,468 J=20.468 kJ

1 J = 0.001 kJ

20.468 kilo Joules is the enthalpy change when one mole of sodium nitrate dissolves.

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Expalin subshells and orbitals
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E

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