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kenny6666 [7]
3 years ago
6

In a gas the kinetic energy is?

Chemistry
1 answer:
Mice21 [21]3 years ago
8 0

Answer:

The kinetic energy of the translational motion of an ideal gas depends on its temperature.

Explanation:

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If you can run 3 miles in 19 minutes. What is your pace in kilometers per hour?
Norma-Jean [14]

Answer:

10.1389

Explanation:

5 0
2 years ago
Calculate the amount in grams of Na2CO3 needed in a reaction with HCl to produce 120g NaCl?
klemol [59]
The balanced chemical reaction is written as :

Na2CO3<span> + 2HCl === 2NaCl + H2O + CO2
</span>
We are given the amount of NaCl to be produced from the reaction. This will be the starting point for the calculations. We do as follows:

120 g NaCl ( 1 mol / 58.44 g) ( 1 mol Na2CO3 / 2 mol NaCl)( 105.99 g / 1 mol ) = 1108.82 g Na2CO3 needed
8 0
3 years ago
How man grams of cl2 are consumed to produce 12.0 g of KCl
Korvikt [17]

Answer:

5.71 g

Explanation:

Step 1: Write the balanced equation

2 K + Cl₂ ⇒ 2 KCl

Step 2: Calculate the moles corresponding to 12.0 g of KCl

The molar mass of KCl is 74.55 g/mol.

12.0 g × 1 mol/74.55 g = 0.161 mol

Step 3: Calculate the moles of Cl₂ needed to produce 0.161 moles of KCl

The molar ratio of Cl₂ to KCl is 1:2. The moles of Cl₂ needed are 1/2 × 0.161 mol = 0.0805 mol

Step 4: Calculate the mass corresponding to 0.0805 moles of Cl₂

The molar mass of Cl₂ is 70.91 g/mol.

0.0805 mol × 70.91 g/mol = 5.71 g

8 0
3 years ago
Draw the condensed structural formula for the ester formed when each of the following reacts with methyl alcohol:
Vikki [24]

Answer:

1) HCOOCH3

2) CH3CH2COOCH3

3) CH3CH2CH2CH(CH3)COOCH3

Explanation:

In the reaction between an alcohol and a carboxylic acid, an ester and water are formed. It is analogous to the inorganic neutralization reaction but this reaction is called esterification in organic chemistry. Esters contain the general formula RCOOR where the RCOO moiety was obtained from the acid and the other R moiety was obtained from the alcohol. The -COOR shows the ester linkage in the molecule. The condensed structural formulas shown in the answer reflects these facts.

6 0
3 years ago
In Part A, we saw that the theoretical yield of aluminum oxide is 1.60 mol . Calculate the percent yield if the actual yield of
garri49 [273]

Taking into account definition of percent yield, the percent yield for the reaction is 76.25%.

<h3>Percent yield</h3>

The percent yield is the ratio of the actual return to the theoretical return expressed as a percentage.

The percent yield is calculated as the experimental yield divided by the theoretical yield multiplied by 100%:

percent yield=\frac{actual yield}{theorical yield}x100

where the theoretical yield is the amount of product acquired through the complete conversion of all reagents in the final product, that is, it is the maximum amount of product that could be formed from the given amounts of reagents.

<h3>Percent yield in this case</h3>

In this case, you know:

  • actual yield= 1.22 mol
  • theorical yield= 1.60 mol

Replacing in the definition of percent yields:

percent yield=\frac{1.22 mol}{1.60 mol}x100

Solving:

<u><em>percent yield= 76.25%</em></u>

Finally, the percent yield for the reaction is 76.25%.

Learn more about percent yield:

brainly.com/question/14408642

#SPJ1

4 0
1 year ago
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