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3 years ago

What is the definition for floating

Chemistry

2 answers:

Mariana [72]3 years ago

8 0

The definition for floating is to rest on the surface of a fluid

creativ13 [48]3 years ago

5 0

Answer:

"1. buoyant or suspended in water or air.

2.not settled in a definite place; fluctuating or variable."

Explanation:

Hope this helps! :)

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A mixture of helium, nitrogen and oxygen has a total pressure of 756 mmHg. The partial

Karolina [17]

Answer:

The partial pressure of oxygen in the mixture is 296 mmHg.

Explanation:

The pressure exerted by a particular gas in a mixture is known as its partial pressure. So, Dalton's law states that the total pressure of a gas mixture is equal to the sum of the pressures that each gas would exert if it were alone.

This relationship is due to the assumption that there are no attractive forces between the gases.

So, in this case, the total pressure is:

PT=Phelium + Pnitrogen + Poxygen

You know:

PT= 756 mmHg
Phelium= 122 mmHg
Pnitrogen= 338 mmHg
Poxygen= ?

Replacing:

756 mmHg= 122 mmHg + 338 mmHg + Poxygen

Solving:

756 mmHg - 122 mmHg - 338 mmHg = Poxygen

Poxygen= 296 mmHg

The partial pressure of oxygen in the mixture is 296 mmHg.

6 0

3 years ago

HELP!!!!!!!!!!!!!!!! PRETTY PLEASE !!!!!!!!!!!!!!!!

I am Lyosha [343]

Answer:

B. 75.0 kPa

Explanation:

P1V1/T1=P2V2/T2

(x * 100 L)/(300 K)=(100 kPa * 50.0 L)/(200 K)

x=75.0 kPa

4 0

4 years ago

Read 2 more answers

A cell with normal tonicity is placed in a 200 mm nacl solution. This solution is ________ and the cell will ________.

const2013 [10]

The concentration of a cell is generally 0.15 M (0.9 % NaCl)

As given the solution has concentration = 200mm = 0.02 M

This concentration of solution is less than the concentration of cell

Hence solution is hypotonic (less concentration) and cell will be hypertonic

7 0

4 years ago

In the explosion of a hydrogen-filled balloon, 0.80 g of hydrogen reacted with 6.4 g of oxygen. How many grams of water vapor ar

mylen [45]

0.4 moles H2O x (18.0 g / mole) = 7.2 g H2O

Explanation:

write the values given in the question

In an explosion of hydrogen balloon, 0.80g of hydrogen is reacted with 6.4g of oxygen.

Write the balanced equation

2 H2 + O2 ---> 2 H2O

0.80 g H2 x (1 mole / 2g) = 0.4 moles H2

6.4 g O2 x (1 mole / 32g) = 0.2 moles O2

from balanced equation, 2 moles H2 react with 1 mole O2

therefore

0.4 moles H2 x (1 mole O2 / 2 moles H2) = 0.2 moles O2

since we need 0.2 moles O2 to react with all the H2 and we have exactly that amount, the amounts are said to be

"stoichiometric" and either reactant can be considered limiting

from the balanced equation, 2 moles H2 --> 2 moles H2O.. therefore

0.4 moles H2 x (2 moles H2O / 2 moles H2) = 0.4 moles H2O

Then

0.4 moles H2O x (18.0 g / mole) = 7.2 g H2O

8 0

3 years ago

how many ml of 0.032 molar kmno4 are required to react with 50.0 ml of 0.100 molar h2c2o4 in the presence of excess h2so4

BartSMP [9]

Answer:

62.5 ml of 0.032 M KMnO₄ are required to react with 50.0 ml of 0.100 molar H₂C₂O₄ in the presence of excess H₂SO₄

Explanation:

The balanced reaction is:

2 KMnO₄ + 5 H₂C₂O₄ + 3 H₂SO₄ → K₂SO₄ + 2 MnSO₄ + 8 H₂O + 10 CO₂

By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

KMnO₄: 2 moles
H₂C₂O₄: 5 moles
H₂SO₄: 3 moles
K₂SO₄: 1 mole
MnSO₄: 2 moles
H₂O: 8 moles
CO₂: 10 moles

Molarity or Molar Concentration is the number of moles of solute that are dissolved in a certain volume.

The molarity of a solution is calculated by dividing the moles of the solute by the volume of the solution:

$Molarity=\frac{number of moles of solute}{volume}$

Molarity is expressed in units $\frac{moles}{liter}$

In this case, 50 mL (0.05 L) of 0.1 M H₂C₂O₄ react. So, replacing the data in the definition of molarity:

$0.1 M=\frac{number of moles of solute}{0.05 L}$

Solving:

number of moles of solute= 0.1 M*0.05 L

number of moles of solute= 0.005 moles

So, 0.005 moles of H₂C₂O₄ react. Then you can apply the following rule of three: if by stoichiometry 5 moles of H₂C₂O₄ react with 2 moles of KMnO₄, 0.005 moles of H₂C₂O₄ react with how many moles of KMnO₄?

$moles of KMnO_{4} =\frac{0.005moles of H_{2} C_{2} O_{4}* 2moles of KMnO_{4} }{5moles of H_{2} C_{2} O_{4} }$

moles of KMnO₄= 0.002 moles

Knowing that the molarity of KMnO₄ is 0.032 M, replacing in its definition and solving:

$0.032 M=\frac{0.002 moles}{volume}$

$volume=\frac{0.002 moles}{0.032 M}$

volume= 0.0625 L= 62.5 mL

62.5 ml of 0.032 M KMnO₄ are required to react with 50.0 ml of 0.100 molar H₂C₂O₄ in the presence of excess H₂SO₄

6 0

3 years ago