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mixas84 [53]
3 years ago
12

A soccer player twists her ankle on the field. The atheltic trainer applies an ice bag with 260 g of ice inside. How much heat,

in joules, wil be absorbed, to melt all the ice to 0°C?
Chemistry
1 answer:
LuckyWell [14K]3 years ago
4 0

Answer:

Q = 8.68 × 10⁴ J

Explanation:

We can calculate the heat required to melt a mass of ice, that is, to change it from the solid phase to the liquid phase, at a constant temperature of 0 °C, using the following expression.

Q = ΔH°f × m

where,

  • Q is the heat absorbed
  • ΔH°f is the standard enthalpy of fusion (ΔH°f for water: 334 J/g)
  • m is the mass of ice

Q = ΔH°f × m

Q = 334 J/g × 260 g

Q = 8.68 × 10⁴ J

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Answer:

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3 years ago
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1/2 - 3/7=??????????????????????​
Veseljchak [2.6K]
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3 years ago
The partial pressure of CO2 inside a bottle of soft drink is 4.0 atm at 25°C. The solubility of CO2 is 0.12 mol/L. When the bott
navik [9.2K]
We can solve this problem by using Henry's law. 
Henry's law states that the amount of dissolved gas is proportional to its partial pressure.
C=kP
C is <span>the solubility of a gas.
</span><span>k is Henry's law constant.
</span><span>P is the partial pressure of the gas.
</span>We can calculate the constant from the first piece of information and then use Henry's law to calculate solubility in open drink.
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k=0.03
Now we can calculate the solubility in open drink.
C_o=kP_o&#10;
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Now we need to convert it to g/L. One mol of CO2 is 44.01<span>g. 
</span>The final answer is:
C_o=0.09\cdot 10^{-4}\cdot 44,01=3.4\cdot 10^{-4} \frac{g}{L} 


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3 years ago
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valina [46]
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Answer is D)
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3 years ago
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