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Alexxx [7]
3 years ago
6

A molten sample of 1.00kg of iron with a specific heat of 0.385J/g.K at 1000.K is immersed in a sample of water. If the water ab

sorbs 270 kJ of heat what is the final temperature of the iron?
Chemistry
1 answer:
Schach [20]3 years ago
6 0

Answer:

Final T = 298.7K

Explanation:

In this problem, the heat given for the iron is equal to the heat that water absorbs. Using the equation:

Q = C*m*ΔT

<em>Where Q is heat given = 270000J</em>

<em>C is specific heat of substance = 0.385J/gK</em>

<em>m is mass of iron = 1000g</em>

<em>ΔT is change in temperature = Initial temperature - Final temperature.</em>

<em />

270000J = 0.385J/gK*1000g*(1000K-Final temperature)

701.3J/K = 1000K - Final T

<h3>Final T = 298.7K</h3>
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Using the periodic table, how would you find elements with chemical properties similar to helium?
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a bowl of cereal is at a temperature of 62 fahrenheit then the bowl of cereal thermal energy decreases as soon as mass or not ch
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  53 fahrenheit

<h3>Explanation:</h3>

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What is a solubility?
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A mixture of H2 and water vapor is present in a closed vessel at 20. 00°C. The total pressure of the system is 755. 0 mmHg. The
MAVERICK [17]

The partial stress of H2 is 737.47 mmHg Let's observe the Ideal Gas Law to find out the whole mols.

We count on that the closed vessel has 1L of volume

  • P.V=n.R.T
  • We must convert mmHg to atm. 760 mmHg.
  • 1 atm
  • 755 mmHg (755/760) = 0.993 atm
  • 0.993 m.1L=n.0.082 L.atm/mol.K .
  • 293 K(0.993 atm 1.1L)/(0.082mol.K /L.atm).
  • 293K = n
  • 0.0413mols = n

These are the whole moles. Now we are able to know the moles of water vapor, to discover the molar fraction of it.

  1. P.V=n.R.T
  2. 760 mmHg. 1 atm
  3. 17.5 mmHg (17.5 mmHg / 760 mmHg)=0.0230 atm
  4. 0.0230 m.1L=n.0.082 L.atm/mol.K.293 K(0.0230atm.1L)/(0.082mol.K/L.atm .293K)=n 9.58 × 10 ^ 4 mols = n.
  5. Molar fraction = mols )f gas/general mols.
  6. Molar fraction water vapor =9.58×10^ -four mols / 0.0413 mols
  7. Sum of molar fraction =1
  8. 1 - 9.58 × 10 ^ 4 × mols / 0.0413 ×mols = molar fraction H2
  9. 0.9767 = molar fraction H2
  10. H2 pressure / Total pressure =molar fraction H2
  11. H2 pressure / 55mmHg = =0.9767 0.9767 = h2 pressure =755 mmHg.
  12. 737,47 mmHg.
<h3>What is a mole fraction?</h3>

Mole fraction is a unit of concentration, described to be identical to the variety of moles of an issue divided through the whole variety of moles of a solution. Because it's miles a ratio, mole fraction is a unitless expression.

Thus it is clear that the partial pressure of H2 is 737,47 mmHg.

To learn  more about partial pressure refer to the link :

brainly.com/question/19813237

<h3 />

5 0
2 years ago
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