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pogonyaev
3 years ago
12

Classify each of the following as a pure substance or a mixture; if it is a mixture, state whether it is heterogeneous

Chemistry
1 answer:
Juli2301 [7.4K]3 years ago
6 0

Answer:

(a) Heterogeneous mixture; (b) heterogeneous mixture;

(c) heterogeneous mixture; (d) homogeneous mixture; (e) pure substance.

Explanation:

(a) Concrete

Heterogeneous mixture. Concrete is a mixture of sand, gravel, and crushed stone held together with a cement.

In a heterogeneous mixture, you can see definite boundaries between the various components.  

(b) Tomato juice

Heterogeneous mixture. It consists of water, tomato pulp, salt, and other substances.

(c) Marble

Heterogeneous mixture. It consists mostly of CaCO₃, but it usually contains other substances such as mica, quartz, pyrite, and iron oxides.  

(d) Seawater

Homogeneous mixture. Seawater is an aqueous solution of NaCl along with other ions like Mg²⁺, Ca²⁺ ,and SO₄²⁻.

(e) Iron

Pure substance. Iron is an element. It consists only of Fe atoms.

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PLZ ANSWER IN THE NEXT 24 HOURS MANY POINTS!!!!!!!!
Katen [24]

Answer:

Ununennium.

Explanation:

Ununennium, also known as <em>eka-francium</em> or <em>element 119</em>, is the hypothetical chemical element with symbol <em>Uue</em> <em>and atomic number 119. </em> It's Mass number is [315] (predicted), as we as it is existing on the periodic table hence its symbol: <em>Uue</em>

3 0
3 years ago
Read 2 more answers
At 400 K, the equilibrium constant for the reaction Br2 (g) + Cl2 (g) ↔ 2BrCl (g) is Kp = 7.0. A closed vessel at 400 K is charg
xz_007 [3.2K]

Answer:

(a) The equilibrium partial pressure of BrCl (g) will be greater than 2.00 atm.

Explanation:

Q is the coefficient of the reaction and is calculated the same of the way of the equilibrium constant, but using the concentrations or partial pressures in any moment of the reaction, so, for the reaction given:

Q = (pBrCl)²/(pBr₂*pCl₂)

Q = 2²/(1x1)

Q = 4

As Q < Kp, the reaction didn't reach the equilibrium, and the value must increase. As we can notice by the equation, Q is directly proportional to the partial pressure of BrCl, so it must increase, and be greater than 2.00 atm in the equilibrium.

The partial pressures of Br₂ and Cl₂ must decrease, so they will be smaller than 1.00 atm. And the total pressure must not change because of the stoichiometry of the reaction: there are 2 moles of the gas reactants for 2 moles of the gas products.

Because is a reversible reaction, it will not go to completion, it will reach an equilibrium, and as discussed above, the partial pressures will change.

5 0
3 years ago
What are causes of air pollution
Rudiy27
Solid and liquid particles
7 0
3 years ago
Combine magnesium metal and hydrochloric acid solution. Mg + HCl →
padilas [110]

Answer:

See below.

Explanation:

This will give magnesium chloride solution and hydrogen gas will evolve.

Mg(s) + 2HCl(l) ---> MgCl2(l) + H2(g)

3 0
3 years ago
Separate a mixture of sand, common salt, copper pieces and iron fillings. Also measure the amount of common salt in the mixture.
Neporo4naja [7]

Answer:

Explanation:

This question seeks to test the knowledge of separation techniques.

From the narration in the question, the first separation to be done is the removal of Iron fillings by the use of magnet (magnetic separation). Since Iron is magnetic, the iron fillings will be attracted by the magnet hence removing the iron fillings from the mixture.

The second constituent to be removed will be the copper pieces by the use of a sieve (sieving). Copper pieces have relatively larger sizes than sand and common salt, hence a sieve (which separates particles based on size) can be used to remove the copper pieces from the mixture.

What will be left in the mixture after the processes above will be salt and water. This mixture will have to be dissolved in water; the salt will dissolve in water while the sand will not. After which, filtration will be done to remove the sand which will be collected on the filter paper as filtride and the salt solution will pass through the filter paper as filtrate.

The salt solution can then be evaporated to dryness to retrieve the solid salt from the solution.

The amount of salt in the mixture can then be measured using a weighing balance.

Some of safety measures to be taken during the course of this experiment includes performing the experiment in an airtight and controlled environment. Lab coat and hand gloves should be worn during the course of the experiment. The evaporation to dryness should not be done close to an inflammable material/substance

5 0
3 years ago
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