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zloy xaker [14]
3 years ago
12

How many Moles of NAOH are present in 2.50L of 0.300 M NaOH?

Chemistry
1 answer:
maw [93]3 years ago
8 0
<h3>Answer:</h3>

0.75 moles NaOH

<h3>Explanation:</h3>

We are given;

Volume of NaOH solution = 2.5 Liters

Molarity of NaOH = 0.300 M

We are required to calculate the moles of NaOH

We need to establish the relationship between moles, molarity and volume of a solution.

That would be;

Concentration/molarity = Moles ÷ Volume

Therefore;

Moles = Concentration × Volume

Thus;

Moles of NaOH = 0.300 moles × 2.50 L

                         = 0.75 moles

Therefore, the number of moles of NaOH is 0.75 moles

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Answer:

D. 2NaBr + Cl_2\rightarrow 2NaCl + Br_2

Explanation:

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In this case, for the given set of chemical reactions, it is possible to infer that D. is a categorized as redox due to the following:

Since both chlorine and bromine remain as diatomic gases, their oxidation states in such a form is 0, but as anions with lithium cations they have a charge of - according to the following reaction and half-reactions:

2NaBr + Cl_2\rightarrow 2NaCl + Br_2

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Unlike the other reactions whereas no change in the oxidation states is evidenced.

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3 years ago
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A sample of krypton gas in a container of volume 1.90 L exerts a pressure of 0.553 atm at 21 Celsius. How many moles of gas are
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Explanation:

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n=1.0507/24.1374

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3 years ago
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The vapor pressure of ethanol is 30°C at 98.5 mmHg and the heat of vaporization is 39.3 kJ/mol. Determine the normal boiling poi
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Answer : The normal boiling point of ethanol will be, 348.67K or 75.67^oC

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where,

P_1 = vapor pressure of ethanol at 30^oC = 98.5 mmHg

P_2 = vapor pressure of ethanol at normal boiling point = 1 atm = 760 mmHg

T_1 = temperature of ethanol = 30^oC=273+30=303K

T_2 = normal boiling point of ethanol = ?

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R = universal constant = 8.314 J/K.mole

Now put all the given values in the above formula, we get:

\ln (\frac{760mmHg}{98.5mmHg})=\frac{39300J/mole}{8.314J/K.mole}\times (\frac{1}{303K}-\frac{1}{T_2})

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Hence, the normal boiling point of ethanol will be, 348.67K or 75.67^oC

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3 years ago
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Calculate the ΔHrxn for the following
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Answer:

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The ΔH for the reaction is -103.4 kJ

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