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andrew11 [14]
3 years ago
15

Calculate the mass of dry ice that should be added to the water so that the dry ice completely sublimes away when the water reac

hes 16 ∘c. assume no heat loss to the surroundings.

Chemistry
1 answer:
riadik2000 [5.3K]3 years ago
8 0
There are a lot of missing information in this problem. I've found a similar problem which is shown in the attached picture. Let's just use the information there that we don't have here.

From the principle of conservation of energy:

Heat of dry ice + Heat of water = 0
Heat of dry ice = - Heat of water
(m of dry ice)ΔH = -(m of water)(Cp)(ΔT)
where Cp for water is 4.187 kJ/kg·°C

Hence,
(m of dry ice)(ΔH°g - ΔH°s) = -(Density*Volume)(Cp)(ΔT)
where the density of water is 1 kg/L and the molar mass of dry ice is 44 g/mol.

Then,
(m of dry ice)(-393.5 - -427.4 kJ/mol)(44 g/mol) = -(1 kg/L*12L)(4.187 kJ/kg·°C)(16 - 88 °C)
Solving for m of dry ice,
<em>Mass = 2.43 g of dry ice</em>

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DENIUS [597]

Respuesta:

292 g / mol;

Por favor, consulte la explicación.

Explicación:

El número de átomos de cada elemento en el compuesto: Fe2 (co3) 3.

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Fe2 = 112 g / mol

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Total = 2 + 3 + 9 = 14

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C = 36/292 * 100% = 12,328 * '

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Answer:

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Explanation:

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