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egoroff_w [7]
3 years ago
13

What is the relationship between pressure and temperature? PLEASEEE HELPPP!!!!!

Chemistry
2 answers:
Aleks [24]3 years ago
6 0

Answer:The pressure of a given amount of gas is directly proportional to its absolute temperature, provided that the volume does not change (Amontons's law). The volume of a given gas sample is directly proportional to its absolute temperature at constant pressure (Charles's law).

Explanation:

brainliest?

kotykmax [81]3 years ago
5 0

Answer:

i forgot

Explanation:

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lora16 [44]
Loosely or widely spaced
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3 years ago
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Manganese forms several oxides when combined with oxygen. One of the oxides (Oxide 1) contains 63.2% of Mn and another oxide (Ox
Nina [5.8K]

Explanation:

Defining law of definite proportions, it states that when two elements form more than one compound, the ratios of the masses of the second element which combine with a fixed mass of the first element will always be ratios of small whole numbers.

A. One of the oxides (Oxide 1) contains 63.2% of Mn.

Mass of the oxide = 100g

Mass of Mn = 63.2 g

Mass of O = 100 - 63.2

= 36.8 g

Ratio of Mn to O = 63.2/36.8

= 1.72

Another oxide (Oxide 2) contains 77.5% Mn.

Mass of oxide = 100 g

Mass of Mn = 77.5 g

Mass of O = 100 - 77.5

= 22.5 g

Ratio of Mn to O = 77.5/22.5

= 3.44

Therefore, the ratio of the masses of Mn and O in Oxide 1 and Oxide 2 is in the ratio 1.72 : 3.44, which is also 1 : 2. So the law of multiple proportions is obeyed.

B.

Oxide 1

Mass of Mn per 1 g of O = mass of Mn/mass of O

= 77.5/22.5

= 3.44 g/g of Oxygen.

Oxide 2

Mass of Mn per 1 g of O = mass of Mn/mass of O

= 77.5/22.5

= 3.44 g/g of Oxygen.

3 0
3 years ago
How many neutrons are present in an atom of
Tamiku [17]
There’s going to be 8 neutrons presented
4 0
3 years ago
_H2SO4 + __ B(OH)3 = _ B2(SO4)3 + __ H2O
Nana76 [90]

Answer:

3H2SO4 + 2B(OH)3 -> B2(SO4)3 + 6H2O

Explanation:

3 0
3 years ago
(CO2) (O2) (He) (N2) (CH4) (Imagine these are balloons with the specified gas inside)
valentina_108 [34]

Answer:

Highest speed: He

Lowest speed: CO2

Explanation:

The rms speed (average speed) of the molecules/atoms in an ideal gas is given by:

v=\sqrt{\frac{3RT}{M}}

where

R is the gas constant

T is the absolute temperature of the gas

M is the molar mass of the gas, which is the mass of the gas per unit mole

From the equation, we see that at equal temperatures, the speed of the molecules in the gas is inversely proportional to the molar mass: the higher the molar mass, the lower the speed, and vice-versa.

In this problem, we have 5 gases:

(CO2) (O2) (He) (N2) (CH4)

Their molar mass is:

CO2: 44 g/mol

O2: 16 g/mol

He: 4 g/mol

N2: 14 g/mol

CH4: 16 g/mol

The gas with lowest molar mass is Helium (He): therefore, this is the gas with greatest average speed.

The gas with highest molar mass is CO2: therefore, this is the gas with lowest average speed.

8 0
3 years ago
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