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3 years ago

Explain the concept: Law of Multiple Proportions. Short and simple please

2 answers:

6 0

When 2 elements combine to form more than one compound. The weight of one element combines with a different weight of the other element then are in a ratio of small whole numbers

cricket20 [7]3 years ago

4 0

In chemistry the law of multiple proportions states that if two elements from more than one compound between them then 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 .

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Point M is located at (4, 6) on a coordinate grid. Point M is translated 8 units to the left and 9 units down to create point M′

lorasvet [3.4K]

Answer:

(-4,-4)

Explanation:

7 0

3 years ago

Use the graph to answer these questions. For numerical answers, use correct significant digits.

kykrilka [37]

Answer:

1. Letter  A shows the overall enthalpy of reaction

2. which is equal to kJ 2,538.90kJ

3. Letter  B shows the activation energy for the reaction

4. The activated complex is represented by letter C

Explanation:

1. Letter __ shows the overall enthalpy of reaction

The overall enthalpy of reaction is equal to the change of enthalpy of the substances:

Enthalpy of reaction = ∑ enthalpy of the products - ∑enthalply of the reactants.

The products are shown of the right side of the diagram. They are C₆H₁₂O₆(g) and 6O₂(g).

The reactants are shown of the left side of the diagram. They are 6CO₂(g) and 6H₂O(g).

The arrow labeled A shows the difference between the enthalpies of the products and the reactants; thus this shows the overall enthalpy of reaction.

2. which is equal to kJ__

You must subtract the enthalpy of the iniital state (reactants) from the enthalpy of the final state (products).

Overall enthalpy of reaction = - 1,273.02kJ - ( - 3,811.92kJ)

Overall enthalpy of reaction = 2,538.90kJ

This is a positive change indicating the reaction is endothermic.

3. Letter___shows the activation energy for the reaction

The activation energy is the energy that the reactants must gain for the reaction occurs.

Thus, it is the difference between the maximum energy, indicated by the label C on the graph, and initial state.

That is shown by the arrow labeled B: the reactants must gain the amount of energy indicated by the arrow labeled B to reach the energy of the state labeled C.

4. The activated complex is represented by ____

The activated complex is the intermediate compound formed while the reactants are breaking their bonds and new bonds start to form the products. It is also called transition state.

The activated complex is on the top of the energy diagram because it hat the highest energy. The formation of the activated complex always requires energy (it is an endothermic process). Once it is formed, energy is released and the reactants are formed (this part is exothermic).

Thus, the activated complex is labeled with the letter C.

8 0

4 years ago

Read 2 more answers

What is the name of the molecule below

Yuliya22 [10]

Explanation:

but.......you havent attached a picture?

3 0

3 years ago

Benzene is 92.3% carbon and 7.7% hydrogen. In anexperiment,

Marysya12 [62]

Answer:

The molecular formula of benzene = $C_{6}H_{6}$

Explanation:

$Moles =\frac {Given\ mass}{Molar\ mass}$

% of C = 92.3

Molar mass of C = 12.0107 g/mol

% moles of C = $\frac{92.3}{12.0107}$ = 7.6848

% of H = 7.7

Molar mass of H = 1.00784 g/mol

% moles of H = $\frac{7.7}{1.00784}$ = 7.6401

Taking the simplest ratio for C and H as:

7.6848 : 7.6401

= 1 : 1

The empirical formula is = $CH$

Molecular formulas is the actual number of atoms of each element in the compound while empirical formulas is the simplest or reduced ratio of the elements in the compound.

Thus,

Molecular mass = n × Empirical mass

Where, n is any positive number from 1, 2, 3...

Mass from the Empirical formula = 12+ 1 = 13 g/mol

Molar mass = 78.0 g/mol

So,

Molecular mass = n × Empirical mass

78.0 = n × 13

⇒ n ≅ 6

The molecular formula of benzene = $C_{6}H_{6}$

7 0

4 years ago