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3 years ago

Which is a characteristic of mixtures

Chemistry

2 answers:

Artyom0805 [142]3 years ago

8 0

Answer:

This question is not complete

Explanation:

Mixture is a combination of two or more substances that are physically combined. This combination cannot be represented by a chemical equation. This combination can also be separated by physical processes such as filtration, evaporation and sedimentation.

Mixtures are generally of two major types; homogeneous and heterogeneous.

Homogeneous mixture is a mixture in which it's constituent particles are evenly distributed in the mixture. Examples are salt solution, sugar solution and air.

Heterogeneous mixture is a mixture in which it's constituent particles are not evenly distributed in the mixture. Examples are sand, oil and water solution e.t.c.

barxatty [35]3 years ago

5 0

They are three types of mixtures:
-solutions : they are homogeneous mixtures of 2 or more sub. in a single phase.
-suspensions: if the particles in a solvent are so large that they settle out unless constantly tired, the mixture is called a suspension.
-colloids: particles that are intermediate in size between those of solutions and suspensions form mixtures called colloids.

:)

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What is the percent yield of a reaction in which 51.5 g of tungsten(VI) oxide (WO3) reacts with excess hydrogen gas to produce m

Rus_ich [418]

Answer:

The percent yield of a reaction is 48.05%.

Explanation:

$WO_3+3H_2\rightarrow W+3H_2O$

Volume of water obtained from the reaction , V= 5.76 mL

Mass of water = m = Experimental yield of water

Density of water = d = 1.00 g/mL

$M=d\times V = 1.00 g/mL\times 5.76 mL=5.76 g$

Theoretical yield of water : T

Moles of tungsten(VI) oxide = $\frac{51.5 g}{232 g/mol}=0.2220 mol$

According to recation 1 mole of tungsten(VI) oxide gives 3 moles of water, then 0.2220 moles of tungsten(VI) oxide will give:

$\frac{3}{1}\times 0.2220 mol=0.6660 mol$

Mass of 0.6660 moles of water:

0.666 mol × 18 g/mol = 11.988 g

Theoretical yield of water : T = 11.988 g

To calculate the percentage yield of reaction , we use the equation:

$\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

$=\frac{m}{T}\times 100=\frac{5.76 g}{11.988 g}\times 100=48.05\%$

The percent yield of a reaction is 48.05%.

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Answer:

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IrinaK [193]

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Answer: The balanced half reaction is written below.

Explanation:

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