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KatRina [158]
2 years ago
15

What happens to the air as the stove heats it?

Chemistry
1 answer:
erastova [34]2 years ago
7 0

NOTHING really but as the stove is on with water boiling the air get moist

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What is the number of moles of solute in a 0.3 molal solution containing 0.10 kg of solvent? Don't forget the unit.
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Molality is one way of expressing concentration for solutions. It has units of moles of solute per kg of solvent. From the given values, we easily calculate for the moles of solute by multiplying the mass of solvent to the molality. We do as follows:

moles solute = 0.3 (10) = 3 mol solute


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Will the solubility of CaSO4 in 0.10 Molar CaF2 be smaller than, larger than, or the same as in pure water?
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Determine the value for the following reaction. N2(g) + 3H2(g) → 2NH3(g)+ 22,000 cal ΔH =
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<span>The </span>ΔH value is -22kcal
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How many sugar molecules are in 0.734 mol sugar, C6H12O6? Please explain
Dmitrij [34]
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3 years ago
Calculate the amount of heat released when 27.0 g H2O is cooled from a liquid at 314 K to a solid at 263 K. The melting point of
BlackZzzverrR [31]

Answer : The amount of heat released, 45.89 KJ

Solution :

Process involved in the calculation of heat released :

(1):H_2O(l)(314K)\rightarrow H_2O(l)(273K)\\\\(2):H_2O(l)(273K)\rightarrow H_2O(s)(273K)\\\\(3):H_2O(s)(273K)\rightarrow H_2O(s)(263K)

Now we have to calculate the amount of heat released.

Q=[m\times c_{p,l}\times (T_{final}-T_{initial})]+\Delta H_{fusion}+[m\times c_{p,s}\times (T_{final}-T_{initial})]

where,

Q = amount of heat released = ?

m = mass of water = 27 g

c_{p,l} = specific heat of liquid water = 4.184 J/gk

c_{p,s} = specific heat of solid water = 2.093 J/gk

\Delta H_{fusion} = enthalpy change for fusion = 40.7 KJ/mole = 40700 J/mole

conversion : 0^oC=273k

Now put all the given values in the above expression, we get

Q=[27g\times 4.184J/gK\times (314-273)k]+40700J+[27g\times 2.093J/gK\times (273-263)k]

Q=45896.798J=45.89KJ     (1 KJ = 1000 J)

Therefore, the amount of heat released, 45.89 KJ

7 0
3 years ago
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