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max2010maxim [7]
2 years ago
14

State the two laws of chemical combination.​

Chemistry
1 answer:
larisa86 [58]2 years ago
4 0
  • Law of Conservation of Mass. In simple terms, this law states that matter can neither be created nor destroyed.
  • Law of Definite Proportions.
  • Law of Multiple Proportions.
  • Gay Lussac's Law of Gaseous Volumes
  • Avogadro's Law.

Brainliest me dear :)

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Electrical energy is used to turn the blades of a fan. The amount of energy transformed is seen here: 750 J electrical energy is
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B) It was transformed into 350 J of heat energy.

Explanation:

The remaining 350J of energy must have been transformed into 350J of heat energy.

A fan works by converting electrical energy into heat energy.

  • According to the third law of thermodynamics "no system is 100% efficient". The conversion of the energy from one form to another involves a lost in energy.
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6 0
3 years ago
THE ANSWER IS <br> Magnesium hydroxide (Mg(OH)2): 58.33<br><br> Iron(III) oxide (Fe2O3): 159.70
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Answer:

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5 0
3 years ago
A compound is composed of C, H and O. A 1.621 g sample of this compound was combusted, producing 1.902 g of water and 3.095 g of
vlada-n [284]

Answer: The molecular of the compound is, C_2H_3O

Explanation:

The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:

C_xH_yO_z+O_2\rightarrow CO_2+H_2O

where, 'x', 'y' and 'z' are the subscripts of Carbon, hydrogen and oxygen respectively.

We are given:

Mass of CO_2=3.095g

Mass of H_2O=1.902g

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 3.095g of carbon dioxide, \frac{12}{44}\times 3.095=0.844g of carbon will be contained.

For calculating the mass of hydrogen:

In 18 g of water, 2 g of hydrogen is contained.

So, in 1.902g of water, \frac{2}{18}\times 1.092=0.121g of hydrogen will be contained.

For calculating the mass of oxygen:

Mass of oxygen in the compound = (1.621)-[(0.844)+(0.121)]=0.656g

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

Step 1: Converting the given masses into moles.

Moles of Carbon =\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{0.844g}{12g/mole}=0.0703moles

Moles of Hydrogen = \frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.121g}{1g/mole}=0.121moles

Moles of Oxygen = \frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{0.656g}{16g/mole}=0.041moles

Step 2: 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 0.041 moles.

For Carbon = \frac{0.0703}{0.041}=1.71\approx 2

For Hydrogen  = \frac{0.121}{0.041}=2.95\approx 3

For Oxygen  = \frac{0.041}{0.041}=1

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : O = 2 : 3 : 1

Hence, the empirical formula for the given compound is C_2H_3O_1=C_2H_3O

The empirical formula weight = 2(12) + 3(1) + 1(16) = 43 gram/eq

Now we have to calculate the molecular formula of the compound.

Formula used :

n=\frac{\text{Molecular formula}}{\text{Empirical formula weight}}

n=\frac{46.06}{43}=1

Molecular formula = (C_2H_3O_1)_n=(C_2H_3O_1)_1=C_2H_3O

Therefore, the molecular of the compound is, C_2H_3O

6 0
3 years ago
The process invented in 1864 to reduce the amount of bacteria in liquids and foods by heating them to high temperatures is calle
dlinn [17]
 The key is a process called <span>pasteurization</span>
5 0
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How many atoms of hydrogen in the product of the equation below:
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Answer: 12 atoms

Explanation: the equation has 6H2 i.e

6*2 = 12

6 0
3 years ago
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