Which type of mixture can be separated using a sieve?

1 answer:

5 0

FILTRATION When the substances in a mixture have different particle sizes, they are separated by filtration. The mixture is poured through a sieve or filter. The smaller particles slip through the holes, but the larger particles do not.p

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Will mark brainliest for who is right :) so NO GESSING

dem82 [27]

Answer:

Matter undergoes a change. The changes are of two types: Physical and chemical change.

A physical change is a change that involves only a change in the physical state of matter. Its chemical properties remain the same. Usually increasing the temperature or applying pressure or both bring about a physical change. On reversing the condition, that is reducing the temperature or reducing the pressure or both, the original state of matter is restored. In other words, physical changes are reversible.

A chemical change is a change that involves a change in the chemical composition of matter. A new substance is formed. In a chemical change, new chemical and physical properties of the substance are formed. In a chemical change, the chemical and physical properties of the substance formed will be different from the original substance.

7 0

3 years ago

. In the nuclear industry, chlorine trifluoride is used to prepare uranium hexafluoride, a volatile compound of uranium used in

valentina_108 [34]

Answer : The the rate expression will be:

$Rate=-\frac{d[Cl_2]}{dt}=-\frac{1}{3}\frac{d[F_2]}{dt}=+\frac{1}{2}\frac{d[ClF_3]}{dt}$

Explanation :

The general rate of reaction is,

$aA+bB\rightarrow cC+dD$

Rate of reaction : It is defined as the change in the concentration of any one of the reactants or products per unit time.

The expression for rate of reaction will be :

$\text{Rate of disappearance of A}=-\frac{1}{a}\frac{d[A]}{dt}$

$\text{Rate of disappearance of B}=-\frac{1}{b}\frac{d[B]}{dt}$

$\text{Rate of formation of C}=+\frac{1}{c}\frac{d[C]}{dt}$

$\text{Rate of formation of D}=+\frac{1}{d}\frac{d[D]}{dt}$

$Rate=-\frac{1}{a}\frac{d[A]}{dt}=-\frac{1}{b}\frac{d[B]}{dt}=+\frac{1}{c}\frac{d[C]}{dt}=+\frac{1}{d}\frac{d[D]}{dt}$

From this we conclude that,

In the rate of reaction, A and B are the reactants and C and D are the products.

a, b, c and d are the stoichiometric coefficient of A, B, C and D respectively.

The negative sign along with the reactant terms is used simply to show that the concentration of the reactant is decreasing and positive sign along with the product terms is used simply to show that the concentration of the product is increasing.

Now we have to determine the rate expressions for this given reaction.

The given balanced equations is:

$Cl_2(g)+3F_2(g)\rightarrow 2ClF_3(g)$