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Alexandra [31]
2 years ago
12

Start four fundamental laws of chemical Combinations and the scientist that stated each below (1) Law of Conseriation of mass (2

) Law of Definite proporsionis (3)Law of multiple proportions (4)Law of reciprocal propertion​
Chemistry
1 answer:
kirza4 [7]2 years ago
8 0

Explanation:

Law of conservation of matter/mass

the law of conservation of mass states that matter cannot be created nor destroyed but can be changed from one form to another.

by Antoine Lavoisier

Law of multiple proportions

the law of multiple proportions states that if two elements, A and B combine to form more than one chemical compound, the various masses of element A, which combine separately with a fixed mass of the other element B are in simple multiple ratios.

by chemist John Dalton

Law of reciprocal proportion

the law of reciprocal proportion states that the masses of several elements A, B, C

which combine separately with a fixed mass of another element D are the same as or simple multiples of, the masses in which A, B, and C themselves combine.

by Jeremias Richter

Law of definite proportions

the law of definite proportions states that all pure samples of a particular chemical combined contain similar elements combined in the same proportion by mass.

by Joseph Proust

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How many moles of HCl would react with 37.1 mL of 0.138 M Sr(OH)2
Lena [83]

Answer is: 0.102 moles of HCl would react.

Balanced chemical reaction:

2HCl(aq) + Sr(OH)₂ → SrCl₂(aq) + 2H₂O(l).

V(Sr(OH)₂) = 37.1 mL ÷ 1000 mL/L.

V(Sr(OH)₂) = 0.0371 L; volume of the strontium hydroxide solution.

c(Sr(OH)₂) = 0.138 M; molarity of the strontium hydroxide solution.

n(Sr(OH)₂) = c(Sr(OH)₂) · V(Sr(OH)₂).

n(Sr(OH)₂) = 0.0371 L · 0.138 mol/L.

n(Sr(OH)₂) = 0.0051 mol; amount of the strontium hydroxide.

From balanced chemical reaction: n(Sr(OH)₂) : n(HCl) = 1 : 2.

n(HCl) = 2 · n(Sr(OH)₂).

n(HCl) = 2 · 0.0051 mol.

n(HCl) = 0.0102 mol; amount of the hydrochloric acid.

5 0
3 years ago
If the enthalpy value for a reaction is negative, what does that indicate about the reaction?
likoan [24]
This indicates that the reaction is exothermic meaning that it releases heat/energy
7 0
3 years ago
Read 2 more answers
Given 8.25 g of butanoic acid and excess ethanol, how many grams of ethyl butyrate would be synthesized, assuming a complete 100
mash [69]

Answer:

              10.87 g of Ethyl Butyrate

Solution:

The Balance Chemical Equation is as follow,

   H₃C-CH₂-CH₂-COOH + H₃C-CH₂-OH  →  H₃C-CH₂-CH₂-COO-CH₂-CH₃ + H₂O

According to equation,

    88.11 g (1 mol) Butanoic Acid produces  =  116.16 g (1 mol) Ethyl Butyrate

So,

           8.25 g Butanoic Acid will produce  =  X g of Ethyl Butyrate

Solving for X,

                      X =  (8.25 g × 116.16 g) ÷ 88.11 g

                      X =  10.87 g of Ethyl Butyrate

8 0
3 years ago
The pressure of a fixed mass of gas is increased from 100 kPa to 600 kPa at a constant temperature. The new volume of the gas is
Dima020 [189]

Answer: The new volume of the gas is smaller.

Explanation:

Volume and pressure are inversely proportional (as one goes up, one goes down). So as you increase the pressure, you decrease the volume.

7 0
2 years ago
Determine the empirical and molecular formula for chrysotile asbestos. Chrysotile has the following percent composition: 28.03%
nlexa [21]

<u>Answer:</u> The empirical and molecular formula of chrysotile is Mg_3Si_2H_3O_4 and Mg_6Si_4H_6O_{16}

<u>Explanation:</u>

We are given:

Percentage of Mg = 28.03 %

Percentage of Si = 21.60 %

Percentage of H = 1.16 %

Percentage of O = 49.21 %

Let the mass of compound be 100 g. So, percentages given are taken as mass.

Mass of Mg = 28.03 g

Mass of Si = 21.60 g

Mass of H = 1.16 g

Mass of O = 49.21 g

To formulate the empirical formula, we need to follow some steps:

  • <u>Step 1:</u> Converting the given masses into moles.

Moles of Magnesium = \frac{\text{Given mass of Magnesium}}{\text{Molar mass of Magnesium}}=\frac{28.03g}{24g/mole}=1.17moles

Moles of Silicon = \frac{\text{Given mass of Silicon}}{\text{Molar mass of Silicon}}=\frac{21.06g}{28g/mole}=0.752moles

Moles of Hydrogen = \frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{1.16g}{1g/mole}=1.16moles

Moles of Oxygen = \frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{49.21g}{16g/mole}=3.07moles

  • <u>Step 2:</u> Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.752 moles.

For Magnesium = \frac{1.17}{0.752}=1.5

For Silicon = \frac{0.752}{0.752}=1

For Hydrogen = \frac{1.16}{0.752}=1.5

For Oxygen = \frac{3.07}{0.485}=4.08\approx 4

To convert the mole ratios into whole numbers, we multiply individual mole ratios by 2

Mole ratio of Magnesium = (2 × 1.5) = 3

Mole ratio of Silicon = (2 × 1) = 2

Mole ratio of Hydrogen = (2 × 1.5) = 3

Mole ratio of Oxygen = (2 × 4) = 8

  • <u>Step 3:</u> Taking the mole ratio as their subscripts.

The ratio of Mg : Si : H : O = 3 : 2 : 3 : 8

The empirical formula for the given compound is Mg_3Si_2H_3O_8

For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is :

n=\frac{\text{Molecular mass}}{\text{Empirical mass}}

We are given:

Mass of molecular formula = 520.8 g/mol

Mass of empirical formula = [(24 × 3) + (28 × 2) + (1 × 3) + (16 × 8)] = 259 g/mol

Putting values in above equation, we get:

n=\frac{520.8g/mol}{259g/mol}=2

Multiplying this valency by the subscript of every element of empirical formula, we get:

Mg_{(3\times 2)}Si_{(2\times 2)}H_{(3\times 2)}O_{(8\times 2)}=Mg_6Si_4H_6O_{16}

Hence, the empirical and molecular formula of chrysotile is Mg_3Si_2H_3O_4 and Mg_6Si_4H_6O_{16}

5 0
3 years ago
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