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finlep [7]
3 years ago
11

When magnesium hydroxide reacts with nitric acid, it produces magnesium nitrate and water

Chemistry
1 answer:
shtirl [24]3 years ago
7 0

It can be shown that matter is neither created nor destroyed in a chemical reaction by taking a critical look at the each atom in both sides of the reaction (reactant and product sides).

1 atom of Mg started the reaction and 1 atom is also present in the products.

8 atoms of O are present in the reactants and 8 is also present in the products.

4 H atoms are present in the reactants and 4 are also present in the products.

2 N atoms are present in the reactants and 2 are also in the products.

In other words, the total number of each atom that is present in the reactants are also present in the product. Nothing has been lost during the reaction, although, the forms of each atom might have changed.

More on the law of conservation of matter can be found here: brainly.com/question/20635180

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During the hot summer days, there is a lot more water in the air. This is due to which change of state?
Zarrin [17]
With the evaporation
5 0
3 years ago
Molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement of __________.A) the law of multiple
fgiga [73]

Answer:

The correct answer is B.

Explanation:

The molecule of water has 2 atoms of hydrogen and 1 atom of oxygen.

The ratio of masses are given as:

2\times 1 g/mol: 1\times 16 g/mol= 1 : 8

This illustrates the law of definite proportions which is also known as law of constant compositions .

The law states that 'the elements combining to form compound always combine in a fixed ratio by their mass.'

Whereas :

Law of multiple proportion states that when two elements combine with each other to form more than one compounds , the mass of one element with respect to the fixed mass of another element are in ratio of small whole numbers.

Law of conservation of mass states that mass can neither be created nor be destroyed but it can only be transformed from one form to another form.

In a balanced chemical reaction ,total mass on the reactant side must be equal to the total mass on the product side.

Law of conservation of energy states that energy can neither be created nor be destroyed but it can only be transformed from one form to another form.

7 0
3 years ago
PLEASE HELP PLEASE HELP PLEASE HELP PLEASE HELP PLEASE HELP PLEASE HELP PLEASE HELP PLEASE HELP PLEASE HELP PLEASE HELP PLEASE H
Goryan [66]
100 m = 0.1 km
9.58 sec = 9.58/3600 = 0.00266 hr
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Can you mark it brainliest?
4 0
2 years ago
A mixture of gases with a pressure of 800.0 mm hg contains 60% nitrogen and 40% oxygen by volume. What is the partial pressure o
larisa86 [58]

Answer:

  • <em>The partial pressure of oxygen in the mixture is</em><u> 320.0 mm Hg</u>

Explanation:

<u>1) Take a base of 100 liters of mixture</u>:

  • N: 60% × 100 liter  = 60 liter

  • O: 40 % × 100 liter = 40 liter.

<u>2) Volume fraction:</u>

At constant pressure and temperature, the volume of a gas is proportional to the number of molecules.

Then, the mole ratio is equal to the volume ratio. Callin n₁ and n₂, the number of moles of nitrogen and oxygen, respectively, and V₁, V₂ the volume of the respective gases you can set the proportion:

  • V₁ / V₂ = n₁ / n₂

That means that the mole ratio is equal to the volume ratio, and the mole fraction is equal to the volume fraction.

Then, since the law of partial pressures of gases states that the partial pressure of each gas is equal to the mole fraction of the gas multiplied by the total pressure, you can draw the conclusion that the partial pressure of each gas is equal to the volume fraction of the gas in the mixture multiplied by the total pressure.

Then calculate the volume fractions:

  • Volume fraction of a gas = volume of the gas / volume of the mixture

  • N: 60 liter / 100 liter = 0.6 liter

  • V: 40 liter / 100 liter = 0.4 liter

<u>3) Partial pressures:</u>

These are the final calculations and results:

  • Partial pressure = volume fraction × total pressure

  • Partial pressure of N = 0.6 × 800.0 mm Hg = 480.0 mm Hg

  • Partial pressure of O = 0.4 × 800.0 mm Hg = 320.0 mm Hg
8 0
3 years ago
45.7 grams of calcium chloride reacts with an excess of aluminum oxide. How many grams of aluminum chloride will be produced
damaskus [11]
Molar mass (CaCl2) = 40.1 +2*35.5 = 111.1 g/mol
Molar mass (AlCl3) = 27.0 +3*35.5= 133.5 g/ mol

                                               
3CaCl2+Al2O3 -------->3CaO +2AlCl3
mole from reaction              3 mol                                              2 mol
mass from reaction         3mol* 111.1g/mol                             2 mol*133.5g/mol
                                               333.3 g                                            267.0 g
mass from problem              45.7 g                                               x g

Proportion:
  333.3 g  CaCl2  -------   267.0 g AlCl3
  45.7 g   CaCl2   --------   x g    AlCl3

x=45.7*267.0/333.3= 36.6 g AlCl3
5 0
3 years ago
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