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3 years ago

Iron (III) oxide - what does the III mean?

Chemistry

1 answer:

Aleonysh [2.5K]3 years ago

7 0

Answer:

The iron is in the +3 oxidation state, which is what the III means.

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cuantos gramos de oxígeno necesarios para que reaccionen completamente 28 gramos de etanol (c2h5oh) en la reaccion de combustion

tigry1 [53]

Answer:

I dont speak this language sorry :(

Explanation:

4 0

3 years ago

2. (2 pts) How would you prepare 1.5 liters of 2 M KCI (MW=74.55 g/mol)

ra1l [238]

Answer:

Dissolve 226 g of KCl in enough water to make 1.5 L of solution

Explanation:

1. Calculate the moles of KCl needed

$n = \text{1.5 L} \times \dfrac{\text{2 mol}}{\text{1 L}}= \text{3.0 mol}$

2. Calculate the mass of KCl

$m = \text{3.0 mol} \times \dfrac{\text{74.55 g}}{\text{1 mol}}= \text{224 g}$

3. Prepare the solution

Measure out 224 g of KCl.
Dissolve the KCl in a few hundred millilitres of distilled water.
Add enough water to make 1.5 L of solution. Mix thoroughly to get a uniform solution.

8 0

3 years ago

How many grams of oxygen can be obtained from 250. grams of KCIO3?

guapka [62]

Answer:

Keep it simple. If all the oxygen contained in the 200 grams of potassium chlorate is produced in the decomposition, then all we have to do is find out how many grams of oxygen are there in the 200 grams. This we can do by calculating the ratio of oxygen mass to the whole. Using 39.1 for potassium, 35.45 for chlorine and 3 times 16, or 48 for the oxygen, we get a total of 122.55 grams per mole for potassium chlorate, of which 48 grams are oxygen. This ratio is 48/122.55. This ratio times the original 200 grams of the compound, gives us 78.34 grams of oxygen produced.

Explanation:

3 0

3 years ago

He molecular formula mass of this compound is 180 amu . what are the subscripts in the actual molecular formula?

mezya [45]

I can't actually answer this one if the empirical formula is not given. Luckily, I've found a similar problem from another website. The problem is shown in the picture attached. It shows that the empirical formula is CH₂O. Let's calculate the molar mass of the empirical formula.

Molar mass of E.F = 12 + 2(1) + 16 = 30 g/mol

Then, let's divide this to the molar mass of the molecular formula.
Molar mass of M.F/Molar mass of E.F = 180/30 = 6

Therefore, let's multiply 6 to each subscript in the empirical formula to determine the actual molecular formula.
<em>Actual molecular formula = C₆H₁₂O₆</em>

5 0

3 years ago

How do you think the amount of a material affects its tendency to sink or float? <br> ASAP

Ksivusya [100]

Answer:

it dependes on the material

Explanation:

what is the material

3 0

3 years ago