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inessss [21]
3 years ago
9

How do I identify polar bonds?

Chemistry
2 answers:
pantera1 [17]3 years ago
7 0
Identify<span> each </span>bond<span> as either </span>polar<span> or nonpolar.</span>
scoundrel [369]3 years ago
6 0
This website can help you. <span>preparatorychemistry.com/Bishop_molecular_polarity.htm</span>
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The chemical agent or hazardous material that interferes with the body's ability to transfer oxygen to the cells is:
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3 years ago
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La aspirina se prepara haciendo reaccionar ácido salicílico con exceso de anhídrido etanoico. En un experimento, 50.05 g de ácid
Tanya [424]

La aspirina se prepara haciendo reaccionar ácido salicílico con exceso de anhídrido etanoico. En un experimento, 50.05 g de ácido salicílico se convirtieron en 55.45 g de aspirina. ¿Cuál fue el porcentaje de rendimiento?

<em>In English:</em>

Aspirin is prepared by reacting salicylic acid with excess ethanoic anhydride. In one experiment, 50.05 g of salicylic acid was converted to 55.45 g of aspirin. What was the yield percentage?

Answer:

el rendimiento porcentual para la cantidad dada de ácido salicílico es 84.99 %

<em>In English:</em>

<em>the percent yield for the given amount of salicylic acid is </em><em>84.99%</em>

<em></em>

Explanation:

La ecuación química equilibrada para la reacción se puede escribir como:

C₇H₆O₃ + C₄H₆O₃    →    C₉H₈O₄ + HC₂H₃O₂

Para la reacción mostrada arriba; El reactivo limitante de la reacción es el ácido salicílico. Ahora; calcular el porcentaje de rendimiento; se espera que primero determinemos el rendimiento teórico de la reacción.

Entonces; la fórmula para calcular el porcentaje de rendimiento: \mathbf {= \frac{actual \ yield }{theoretical \ yield } *100 }  

El rendimiento teórico se determina de la siguiente manera:

50.05 g * 1 mol / 138.21 g / mol de C₇H₆O₃ * 1 mol de C₉H₈O₄ / 1 mol de C₇H₆O₃ * 180.157 g / mol de C₉H₈O₄ = 65.24 g de C₉H₈O₄

Porcentaje de rendimiento \mathbf {= \frac{55.45 }{65.24 } *100 }

Porcentaje de rendimiento = 84.99%

Por lo tanto, el porcentaje de rendimiento para la cantidad dada de ácido salicílico es 84.99%

<em>In English:</em>

<em>The balanced chemical eqaution for the reaction can be written as:</em>

<em>C₇H₆O₃ + C₄H₆O₃    →    C₉H₈O₄ + HC₂H₃O₂</em>

<em>For the reaction shown above;  The limiting reactant from the reaction is  salicylic acid. Now; to calculate the percentage yield ; we are expected to first determine the theoretical yield of the reaction. </em>

<em>So; the formula for calculating the percentage yield </em>\mathbf {= \frac{actual \ yield }{theoretical \ yield } *100 }<em>  </em>

<em />

<em>The theoretical yield is determined as follows:</em>

<em>50.05 g * 1 mol/ 138.21 g/mol of C₇H₆O₃ * 1 mol of C₉H₈O₄/ 1 mol of C₇H₆O₃ * 180.157 g/mol of C₉H₈O₄ = 65.24 g of C₉H₈O₄ is produced</em>

<em />

<em>Percentage yield </em>\mathbf {= \frac{55.45 }{65.24 } *100 }<em />

<em>Percentage yield = 84.99%</em>

<em />

<em>Thus, the percent yield for the given amount of salicylic acid is </em><em>84.99%</em>

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In 2011, a computer named Watson competed against two humans on a popular television quiz show and won. Watson listened to each
Molodets [167]

Answer:

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Explanation:

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3 years ago
Calculate the average reaction rate of Cl2 consumed using the following information. H2 + Cl2 yields 2 HCl A table with three co
klemol [59]
Answer : Option D) 2.50 X 10^{-3} Mol/(L s)

Explanation: While calculating the average reaction rate for the given reaction in terms of Cl;

H_{2} + Cl_{2}  ----\ \textgreater \  2HCl.

using the rate equation which is;

\frac{-1}{1}\frac{delta [Cl]}{delta t} = 

\frac{- 0.0875 - 0.0625}{10s - 0s} = 2.50 X 10^{-3} Mol/(L s)
5 0
3 years ago
How many significant digits are in the number 125,001?
Yuri [45]
The number of significant digits in the number 125,001 are: <span>6. 

</span>Significant digits are always:
<span>1. non-zero
</span>2. <span>Any zeros between two significant digits are significant (for example 5 and 1)
</span>3. <span>A final zero or trailing zeros in the decimal portion only are significant.

Hope I helped!</span>
5 0
3 years ago
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