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mars1129 [50]
3 years ago
10

0.1005 liters is the same as: A. 0.0001005 cm3 B.0.1005 cm3 C.100.5 cm3 D.0.01005 cm3 and A. 0.01005 mL B. 0.1005 mL C. 0.000100

5 mL D. 100.5 mL
Chemistry
2 answers:
Andreyy893 years ago
4 0

I think it would be C.100.5cm or D.100.5ml hope that helps


Alecsey [184]3 years ago
4 0

The correct answers are: C. 100.5cm³ and D. 100.5 mL


FIRST.

Cubic centimeter (cm³) is the volume made by a cube that is 1 centimeter on each side.

<em>C. 100.5cm³</em>

1L=1000cm^3 \\ \\ So: \\ \\ 0.1005L=1000\times 0.1005cm^3=\boxed{100.5cm^3}


SECOND.

<em>D. 100.5 mL</em>

1 cubic centimeter is equal to 1mL, which is one-thousandth of a liter. So:


1L=1000mL \\ \\ So: \\ \\ 0.1005L=1000\times 0.1005mL=\boxed{100.5mL}

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How do different stimuli affect the survival behavior of an organism?
Vlad [161]
Organisms change their behavior in responses to changes in the environment.

All living things can respond to stimuli in the exterior environment, it is a form of energy-light waves or sound vibrations, From what they sense they will make necessary changes to their diet and or where they are located. Such as winter weather which is a type stimuli will cause some animals to start talking.
6 0
3 years ago
How many grams of Cu(OH)2 will precipitate when excess NaOH solution is added to 46.0 mL of 0.584 M CuSO4
Slav-nsk [51]
<h3>Answer:</h3>

2.624 g

<h3>Explanation:</h3>

The equation for the reaction is given as;

  • CuSO₄(aq) + 2NaOH(aq) → Cu(OH)₂(s) + Na₂SO₄(aq)
  • Volume of CuSO₄ as 46.0 mL;
  • Molarity of CuSO₄ as 0.584 M

We are required to calculate the mass of Cu(OH)₂ precipitated

  • We are going to use the following steps;
<h3>Step 1: Calculate the number of moles of CuSO₄ used</h3>

Molarity = Number of moles ÷ Volume

To get the number of moles;

Moles = Molarity × volume

          = 0.584 M × 0.046 L

          = 0.0269 moles

<h3>Step 2: Calculate the number of moles of Cu(OH)₂ produced </h3>
  • From the equation 1 mole of CuSO₄ reacts to give out 1 mole of Cu(OH)₂
  • Therefore; Mole ratio of CuSO₄ to Cu(OH)₂ is 1 : 1.

Thus, Moles of CuSO₄ = Moles of Cu(OH)₂

Hence, moles of Cu(OH)₂ = 0.0269 moles

<h3>Step 3: Calculate the mass of Cu(OH)₂</h3>

To get mass we multiply the number of moles with the molar mass.

Mass = Moles × Molar mass

Molar mass of Cu(OH)₂ is 97.561 g/mol

Therefore;

Mass of Cu(OH)₂ = 0.0269 moles × 97.561 g/mol

                           = 2.624 g

Thus, the mass of Cu(OH)₂ that will precipitate is 2.624 g

3 0
3 years ago
QUICK PLEASE
Trava [24]

Answer: 2.52 M

Explanation:

The product of molarity (moles/litre) and volume in litres yields moles, and the numbers of moles in two solutions means dilute and concentrated are equal, which is expressed by the following equation: 

M_1V_1=M_2V_2

$$Given that\\M $1=12.0 \mathrm{M}$ or mole $/ \mathrm{L}$\\$\mathrm{V} 1=420 \mathrm{ml}$\\$\mathrm{M} 2=$ ?\\$\mathrm{V} 2=2.0 \mathrm{~L}$ or $2000 \mathrm{ml}$\\\\$\mathrm{M} 1 \mathrm{~V} 1=\mathrm{M} 2 \mathrm{~V} 2$\\$\mathrm{M} 2=\mathrm{M} 1 \mathrm{~V} 1 / \mathrm{V} 2$\\$=12.0 * 420 / 2000$\\$=2.52 \ \mathrm{M}$

3 0
2 years ago
What is the name of this compound?<br> CH3CH2OCH2CH2CH3
WARRIOR [948]

The name of this compound is Ethyl propyl ether, CH3CH2OCH2CH2CH3 stands for Ethyl propyl ether.

8 0
4 years ago
C. What is oxidized in the reaction? What is reduced? (2 points)
Rina8888 [55]

Answer:

Oxidation: a type of chemical reaction where one or more electrons are lost.

Oxidation State / Number: a number assigned to an atom describing its degree of oxidation, meaning how many electrons it has gained or lost.

Reduction: a type of chemical reaction where one or more electrons are gained.

Oxidation-Reduction Reaction: a chemical reaction where oxidation and reduction occurs simultaneously

Explanation:

Reduction always occurs at cathode

Oxidation always occurs in anode

These two process occurs in same way independent of nature of cell whether voltaic or electrolytic.

6 0
2 years ago
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