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ycow [4]
3 years ago
8

A chemist adds 370.0mL of a 1.41/molL potassium iodide KI solution to a reaction flask. Calculate the millimoles of potassium io

dide the chemist has added to the flask. Be sure your answer has the correct number of significant digits.
Chemistry
1 answer:
Gwar [14]3 years ago
3 0

Answer: The millimoles of potassium iodide the chemist has added to the flask is 522 millimoles.

Explanation:

Given: Volume of KI = 370.0 mL (1 mL = 0.001 L) = 0.37 L

Molarity of KI solution = 1.41 mol/L

Now, moles of KI (potassium iodide) is calculated as follows.

Moles = Volume \times Molarity \\= 0.37 L \times 1.41 M\\= 0.5217 mol

Convert moles into millimoles as follows.

1 mol = 1000 millimoles

0.5217 mol = 0.5217 mol \times \frac{1000 millimoles}{1 mol} = 521.7 millimoles

This can be rounded off to the value 522 millimoles.

Thus, we can conclude that the millimoles of potassium iodide the chemist has added to the flask is 522 millimoles.

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The solubility of oxygen gas in water at 40 ∘c is 1.0 mmol/l of solution. What is this concentration in units of mole fraction?
juin [17]

The formula for mole fraction is:

mole fraction of solute = \frac{number of moles of solute}{total number of moles of solution}    -(1)

The solubility of oxygen gas = 1.0 mmol/L  (given)

1.0 mmol/L means 1.0 mmol are present in 1 L.

Converting mmol to mol:

1.00 mmol\times \frac{1 mol}{1000 mmol} = 0.001 mol

So, moles of oxygen = 0.001 mol

For moles of water:

1 L of water = 1000 mL of water

Since, the density of water is 1.0 g/mL.

Density = \frac{mass}{volume}

Mass = 1.0 g/ml\times 1000 mL = 1000 g

So, the mass of water is 1000 g.

Molar mass of water = 18 g/mol.

Number of moles of water = \frac{1000 g}{18 g/mol} = 55.55 mol

Substituting the values in formula (1):

mole fraction = \frac{0.001}{55.55+0.001}

mole fraction = 1.8\times 10^{-5}

Hence, the mole fraction is 1.8\times 10^{-5}.

7 0
3 years ago
Which substance contains bonds that involve a transfer of electrons from one atom to another
cestrela7 [59]
An ionic bond is a type of chemical bond formed through an electrostatic attraction between two oppositely charged ions. Ionic bonds are formed between a cation, which is usually a metal, and an anion, which is usually a nonmetal. A covalent bond involves a pair of electrons being shared between atoms.
3 0
2 years ago
ELETE
yKpoI14uk [10]

Answer:

5 L

Explanation:

Use Charles law and rearrange formula

Change C to K

- Hope that helped! Please let me know if you need further explanation.

6 0
3 years ago
What is the coefficient of silver in the final, balanced equation for this reaction?
vekshin1

This is an incomplete question, the complete question is attached below.

Answer : The coefficient of silver in the final, balanced equation for this reaction is, 3

Explanation :

Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.

Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.

The given redox reaction is,

Ag^+(aq)+Al(s)\rightarrow Ag(s)+Al^{3+}(aq)

The oxidation-reduction half reaction will be :

Oxidation : Al\rightarrow Al^{3+}+3e^-

Reduction : Ag^{+}+1e^-\rightarrow Ag

In order to balance the electrons, we multiply the reduction reaction by 3 and then added both equation, we get the balanced redox reaction.

The balanced redox reaction will be,

3Ag^+(aq)+Al(s)\rightarrow 3Ag(s)+Al^{3+}(aq)

From the balanced redox reaction we conclude that, the coefficient of silver in the final balanced equation for this reaction is 3.

Hence, the correct option is 3.

8 0
3 years ago
The temperature at which water vapor condenses into liquid water
Marysya12 [62]
Precipitation

100°C
When 1 mol of water vapor at 100°C condenses to liquid water at 100°C, 40.7 kJ of heat are released into the surroundings.
3 0
2 years ago
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