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butalik [34]
3 years ago
9

How much heat would be released by 1.3 kg of water if it's temperature went from 295 k to 274 k

Chemistry
1 answer:
kicyunya [14]3 years ago
4 0

Answer: The energy released will be 114.223 kJ.

Explanation:

To calculate the amount of heat released, we use the formula:

Q= m\times c\times \Delta T

Q = heat gained  or released

m = mass of the substance = 1.3kg = 1300 g   (Conversion factor: 1kg = 1000g)

c = heat capacity of water = 4.184 J/g K

\Delta T={\text{Change in temperature}}=(274-295)K=-21K

Putting values in above equation, we get:  

Q=1300g\times 4.184J/gK\times (-21)K

Q = -114223 Joules  = -114.223 kJ      (Conversion Factor: 1kJ = 1000J)

Negative sign implies heat released.

Hence, heat released by 1.3 kg of water is 114.223kJ.

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NaH_2PO_4, a crystal structure with a short symmetrical hydrogen bond.

<h3>What is Classical bonding?</h3>

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Molten gallium reacts with arsenic to form the semiconductor, gallium arsenide, GaAs, used in light-emitting diodes and solar ce
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Answer:

a) 1.2g of arsenic b) 0.64g of arsenic c) 3.481g of gallium d) 3.806g of gallium e) 2.61g arsenic

Explanation:

The balanced equation is:

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a) mass (gallium)/ molar mass of Ga = 4/ 69.723 = 0.0574mol

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b) repeating the procedure (changing the values)

It will be 0.0574 to 0.06593

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Gallium is in excess by 0.05

Mass of excess gallium = 0.05* 69.723 = 3.481g

d) using the mass given, the new ratio is

0.128: 0.0734

Gallium is in excess by 0.054mol

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Gallium is in excess by 0.0374*69.723 = 2.61g

7 0
3 years ago
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