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3 years ago

Which is a homogeneous mixture

Chemistry

2 answers:

Andrew [12]3 years ago

4 0

Answer:

Explanation:

A mixture is formed by the combination of two or more compounds.

A mixture can be classified into homogeneous or heterogeneous.

If after mixing two or more compounds we can identify the different compounds (phases), that is a heterogeneous mixture. This is easy to notice because the different phases has different characteristics like color, density, states (solid, liquid, gas), etc.

And, if after mixing two or more compounds we cannot see those differents compunds (phases) and we can see just one phase with the same characteristics of color, density, states, etc., that is a homogeneous mixture.

<u>Examples:</u>

- If you mix <u>water and alcohol</u>, we cannot see any difference, the whole mixture has the same color, density and it is liquid, so it is a <u>homogeneous mixture</u>.

- If you mix <u>water and cooking oil</u> in a glass, two different phases appear, with diffrent color and different density. Water phase stays on the bottom of the glass and the cooking oil phase stays on the top of the glass, so it is a <u>heterogeneous mixture</u>.

klemol [59]3 years ago

3 0

A homogeneous mixture is a mixture that is mixed so well together that you cannot see the different components that make up the mixture as the ingredients will not separate out, even over time.

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What is the name of the branched alkane shown below?

lana [24]

Answer:

3-Methyloctane

Explanation:

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3 years ago

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2 Mg(s) + O2(g) → 2 MgO(s) How many moles of O2 ar

TEA [102]

Answer:

1.05 mols of O2 gas

Explanation:

For this type of problem, it's important to understand what the balanced Chemical equation tells us:

<h3><u>Balanced Chemical equations</u></h3>

Let's look at the balanced chemical equation:

$2Mg(s)+O_2(g)-- > 2MgO(s)$

This equation two sides of the reaction arrow. On the left are the reactants (things you start with, and that react during the chemical reaction), and on the right side are products (things that are produced during the chemical reaction that you end with).

The numbers in front of each compound tell how many of molecules are involved for a full reaction without anything left over. A "mol" is a large quantity ( $6.022*10^{23}$ ), in this case, of molecules , since it's unlikely you're only taking a single molecule of each substance (it would be so tiny, you wouldn't even know you were doing the reaction).

So,for every 2 moles of Magnesium used, we'll also need 1 mole of Oxygen, and it will produce 2 moles of Magnesium Oxide.

In a way, during the reaction it's almost like 2 moles of Magnesium is equal to 1 mole of Oxygen and is equal to 2 moles of Magnesium Oxide:

$2 mol Mg(s)=1mol O_2(g)=2molMgO(s)$

From here, we can build some unit ratios, to convert between the known quantity of moles we have, and find the unknown quantity of moles that are requested.

<h3><u>Finding the right unit ratio</u></h3>

We know that we are looking at 2.10 mol of Magnesium, so we want a unit ratio with moles of Mg on the bottom. <u>We want to find moles of O2</u>, <u>so we want a unit ratio of moles of O2 on top</u>.

The unit ratio we want is the middle part of the equation, divided by the left part of the equation.

$2 mol Mg(s)=1mol O_2(g)\\\frac{2 mol Mg(s)}{2 mol Mg(s)}=\frac{1mol O_2(g)}{2 mol Mg(s)}\\1=\frac{1mol O_2(g)}{2 mol Mg(s)}$

Since this quantity is 1, it is a unit ratio and can be multiplied to other things to change their units (for this problem).

<h3><u>Finding the answer</u></h3>

Starting with what we know, and multiplying by our unit ratio:

$2.10 mol Mg(s)*\frac{1mol O_2(g)}{2 mol Mg(s)}=1.05mol O_2(g)$

Notice that the units from the first quantity cancel with the units on the bottom of the fraction, leaving only the unit on top of the fraction ... the exact units we wanted!

So, 1.05mols of O2 would be consumed during the reaction if exactly 2.10moles of Magnesium are burned.

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timofeeve [1]

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Answer:

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Explanation:

brainlest?

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