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BaLLatris [955]
3 years ago
11

If 15 g of C₂H₆ reacts with 60.0 g of O₂, how many moles of water (H₂O) will be produced?

Chemistry
1 answer:
IceJOKER [234]3 years ago
5 0

Answer:

n_{H_2O}=1.5molH_2O

Explanation:

Hello,

In this case, the undergoing chemical reaction is:

2C_2H_6 + 7O_2 \rightarrow 4CO_2 + 6H_2O

Next, we identify the limiting reactant by computing the available moles of ethane and the moles of ethane consumed by 60.0 grams of oxygen:

n_{C_2H_6}^{available}=15g*\frac{1mol}{30g} =0.50molC_2H_6\\n_{C_2H_6}^{reacted}=60.0gO_2*\frac{1molO_2}{32gO_2}*\frac{2molC_2H_6}{7molO_2} =0.536molC_2H_6

Thus, we notice there are less available moles, for that reason, the ethane is the limiting reactant. Finally, we can compute the produced moles of water by:

n_{H_2O}=0.50molC_2H_6*\frac{6molH_2O}{2molC_2H_6}\\\\n_{H_2O}=1.5molH_2O

Best regards.

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50 gramos de soluto a temperatura ambiente en un recipiente de 100ml de agua, pero el solito se acumulaba en el fondo. La calent
Sveta_85 [38]

Answer:

  • <u><em>Saturated</em></u>

<u><em></em></u>

Explanation:

Translation:

  • <em>50 grams of solute at room temperature in a 100ml container of water, but the solute accumulated at the bottom. He heated it allowing it to dissolve just an additional 10 grams of solute. What solution did you get? Oversaturated, unsaturated, saturated or diluted</em>

<em />

<h2>Solution</h2>

A<em> saturated</em> <em>solution</em> contains the maximum amount of solute that it can dissolve at the given temperature and pressure.

If you add more solute than that it will not get <em>dissolved</em> but the extra solute will remain as a solid at the<em> bottom</em> of the <em>solution</em>.

The fact that, for the <em>solution</em> with 50 grams of solute, the <em>solute accumulated</em> at the <em>bottom</em> means that it could not dissolve more, so the solution was saturated.

By <em>heating</em> the solution it was able to <em>dissolve</em> more <em>solute </em>but the fact that yeat some <em>grams</em> were undissolved means that the solution was still saturated at the new temperature.

<em>Oversaturated</em> is an unstable state at which the solution can dissolve more solute than what the normal solubility permits. That state can be reached only under special procedures which would require a different description.

Thus, you get a <em>saturated solution</em>.

6 0
3 years ago
Which statements correctly describe the decay rates of radioactive isotopes?
storchak [24]

Answer: b} The exact time when an individual atom will decay can be accurately predicted.

c} After each half-life, the amount of radioactive material is reduced by half.

Explanation:

All radioactive decay  follows first order kinetics.

Rate law expression for first order kinetics is given by:

t=\frac{2.303}{k}\log\frac{a}{a-x}

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t = time taken for decay process

a = initial amount of the reactant

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Expression for calculating half life, which is the time taken by the half of the reactants to decompose is:

t_{1/2}=\frac{0.693}{k}


4 0
3 years ago
Read 2 more answers
What is the empirical formula for a compound if a sample contains 3.72 g of P and 21.28 g of Cl
fenix001 [56]
M(P)=3.72 g
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m(Cl)=21.28 g
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n(P)=m(P)/M(P)
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n(Cl)=m(Cl)/M(Cl)
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The heat of vaporization of a liquid is 84.0 J/g. How many joules of heat would it take to completely vaporize 172 g of this liq
Aliun [14]

Answer:

14,448 J of heat would it take to completely vaporize 172 g of this liquid at its boiling point.

Explanation:

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During the evaporation process, a substance goes from a liquid to a gaseous state and needs to absorb a certain amount of heat from its immediate surroundings, which results in its cooling. The heat absorbed is called the heat of vaporization.

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In this case, being:

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and replacing in the expression Q = m*L you get:

Q=172 g*84 \frac{J}{g}

Q=14,448 J

<u><em>14,448 J of heat would it take to completely vaporize 172 g of this liquid at its boiling point.</em></u>

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