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2 years ago

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What is the heat required to vaporize 650 grams of a liquid with a heat of vaporization of 723 joules/gram?

2 answers:

ANTONII [103]2 years ago

4 0

Answer: 469,950 J

Explanation:

Vaporization heat is the amount of heat energy needed to vaporize an amount of substance at a constant temperature, this is to change the liquid into gas phase. The temperature remains constant during the change of phase because the energy is being used to beat the intermolecular forces that exist in the liquid phase and so the particles (molecules) can separate to change the state from liquid to gas.

The specific vaporization heat is given in units of joules per gram, meaning that to compute the total amount of heat you just need to multiply the specific vaporization heat times the amount of substance:

Heat energy = mass in grams × specific vaporization heat

Heat energy = 650 g × 723 J/g = 469,950 J ← answer,

Ilia_Sergeevich [38]2 years ago

4 0

Hello!

What is the heat required to vaporize 650 grams of a liquid with a heat of vaporization of 723 joules/gram?

We have the following data:

$H_v\:(heat\:of\:vaporization) = 723\:\dfrac{J}{g}$

$q\:(heat) =\:?\:(in\:Joule)$

$m\:(mass) = 650\:g$

We apply the data to the formula, see:

$H_v = \dfrac{q}{m}$

$q = H_v * m$

$q = 723\:\dfrac{J}{\diagup\!\!\!\!g} * 650\:\diagup\!\!\!\!\!g$

$q = 469950 \to \boxed{\boxed{q \approx 470000\:J}}\end{array}}\qquad\checkmark$

_______________________

I Hope this helps, greetings ... Dexteright02! =)

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Effusion makes fluid/gas molecules move to the container with less pressure or larger volume. In diffusion, the movement should work two ways even though one side might receive more. But in effusion, the movement is rather one way.

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Answer:

<u>1. Net ionic equation:</u>

Cl⁻(aq) + Ag⁺(aq) → AgCl(s)

<u />

<u>2. Volume of 1.0M AgNO₃</u>

41ml

Explanation:

1. Net ionic equation for the reaction of NaCl with AgNO₃.

i) Molecular equation:

It is important to show the phases:

(aq) for ions in aqueous solution
(s) for solid compounds or elements
(g) for gaseous compounds or elements

NaCl(aq) + AgNO₃(aq) → AgCl(s) + NaNO₃(aq)

ii) Dissociation reactions:

Determine the ions formed:

NaCl(aq) → Na⁺(aq) + Cl⁻(aq)

AgNO₃(aq) → Ag⁺(aq) + NO₃⁻(aq)

NaNO₃(aq) → Na⁺(aq) + NO₃⁻(aq)

iii) Total ionic equation:

Substitute the aqueous compounds with the ions determined above:

Na⁺(aq) + Cl⁻(aq) + Ag⁺(aq) + NO₃⁻(aq) → AgCl(s) + Na⁺(aq) + NO₃⁻(aq)

iv) Net ionic equation

Remove the spectator ions:

Cl⁻(aq) + Ag⁺(aq) → AgCl(s) ← answer

2. How many mL of 1.0 M AgNO₃ will be required to precipitate 5.84 g of AgCl

i) Determine the number of moles of AgNO₃

The reaction is 1 to 1: 1 mole of AgNO₃ produces 1 mol of AgCl

The number of moles of AgCl is determined using the molar mass:

number of moles = mass in grams / molar mass

molar mass of AgCl = 143.32g/mol

number of moles = 5.84g / (143.32g/mol) = 0.040748 mol

ii) Determine the volume of AgNO₃

molarity = number of moles of solute / volume of solution in liters

1.0M = 0.040748mol / V

V = 0.040748mol / (1.0M) = 0.040748 liter

V = 0.040748liter × 1,000ml / liter = 40.748 ml

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Yes, the chemist can determine which compound is in the sample.

Explanation:

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In 1 mole of K₂O₂, the mass of K is 2 × 39.1 g = 78.2 g and the mass of K₂O₂ is 110.2 g. The mass ratio of K to K₂O₂ is 78.2 g / 110.2 g = 0.710.

If the chemist knows the mass of K and the mass of the sample, he or she must calculate the mass ratio of K to the sample.

If the ratio is 0.830, the compound is pure K₂O.
If the ratio is 0.710, the compound is pure K₂O₂.
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Be sure to answer all parts. Consider the following balanced redox reaction (do not include state of matter in your answers): 2C

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Answer:

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$X\rightarrow X^{n+}+ne^-$

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$X^{n+}+ne^-\rightarrow X$

For the given chemical reaction:

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The half cell reactions for the above reaction follows:

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Reduction half reaction: $2ClO^- + 4H_2O + 2e^-\rightarrow Cl_2 + 2H_2O + 4OH^-$

Thus, the specie which is oxidized is:- $CrO_2^-$

The specie which is reduced is:- $ClO^-$

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3 years ago