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marissa [1.9K]
3 years ago
9

How many moles of iron is needed to react completely with 5.00 moles of sulfur to form iron

Chemistry
1 answer:
Ghella [55]3 years ago
3 0

Answer:

5 moles of Fe(II) are required to react completely with the 5 moles of Sulphur

Explanation:

The balanced equation in this question is

Iron + Sulfur = Iron(II) Sulfide

Fe (II) + S --> Fe(II)S

Thus one mole of sulfur reacts with one mole of Fe(II)

Hence, 5 moles of Fe(II) are required to react completely with the 5 moles of Sulphur

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is it true that in a solution the tiny pieces of one substance are spread equally through the other substance
ziro4ka [17]
Yes this is true otherwise it would not be a solution
3 0
3 years ago
You need to produce a buffer solution that has a pH of 5.31. You already have a solution that contains 10. mmol (millimoles) of
Karolina [17]

Answer:

37 mmol of acetate need to add to this solution.

Explanation:

Acetic acid is an weak acid. According to Henderson-Hasselbalch equation for a buffer consist of weak acid (acetic acid) and its conjugate base (acetate)-

pH=pK_{a}(acetic acid)+log[\frac{mmol of CH_{3}COO^{-}}{mmol of CH_{3}COOH }]

Here pH is 5.31, pK_{a} (acetic acid) is 4.74 and number of mmol of acetic acid is 10 mmol.

Plug in all the values in the above equation:

5.31=4.74+log[\frac{mmol of CH_{3}COO^{-}}{10}]

or, mmol of CH_{3}COO^{-} = 37

So 37 mmol of acetate need to add to this solution.

3 0
3 years ago
Write down examples of some natural acids and natural bases. Also write use of them.
trasher [3.6K]

Answer:

Formic acid, citric acid, Oxalic acid, washing soda, baking soda, etc. can be some examples of natural acids and natural bases. They both have domestic, industrial, and various other purposes.

Explanation:

<h3><u>NATURAL ACIDS</u>:</h3>

There are lots of natural acids present in our nature. Some of them are the following:

> <u>Formic acid</u>

 USE: It is used in the stimulation of oil and gas wells as it is less reactive towards the metal.

> <u>Citric acid</u>

 USE: It is considered as the best rust remover as it doesn't harm the metal just remove the rust.

> <u>Oxalic acid</u>

USE: It easily remove iron and ink stains and that's why it is used as an acid rinsing material in Laundries.

<h3><u>NATURAL BASES</u>:</h3>

There is a variety of natural base found in our nature which founds a lot of uses in day to day life. some of them are the following:

> <u>Washing soda</u>

USE: It is used in commercial detergent mixture to treat hard water.

> <u>Baking soda</u>

USE: It is the best rising agent used mostly in cooking and for domestic purposes like removing stains, etc..

3 0
3 years ago
The atomic mass of Cu is 63.5. Find its electrochemical equivalent​
FrozenT [24]

Answer:

The electrochemical equivalent of copper, Cu, is 3.29015544 × 10⁻⁷ g/C

Explanation:

The given parameters are;

The element for which the electrochemical equivalent is sought = Copper

The atomic mass of copper = 63.5

The electrochemical equivalent, 'Z', of an element or a substance is the mass, 'm', of the element or substance deposited by one coulomb of electricity, which is equivalent to a 1 ampere current flowing for a period of 1 second

Mathematically, we have;

m = Z·I·t = Z·Q

We have;

Cu²⁺ (aq) + 2·e⁻ → Cu

Therefore, one mole of Cu, is deposited by 2 moles of electrons

The charge carried one mole of electrons = 1 Faraday = 96500 C

∴ The charge carried two moles of electrons, Q = 2 × 96500 C = 193,000 C

Given that the mass of an atom of Cu = 63.5 a.m.u., the mass of one mole of Cu, m = 63.5 g

Z = \dfrac{m}{Q} = \dfrac{63.5 \ g}{193,000 \ C} = 3.29015544 \times 10^{-4} \, g \cdot C^{-1}

∴ Z = 3.29015544 × 10⁻⁴ g/C = 3.29015544 × 10⁻⁷ g/C

The electrochemical equivalent of copper, Cu, is Z = 3.29015544 × 10⁻⁷ g/C

7 0
3 years ago
Which statement best describes the main benefit to organisms that reproduce sexually?
8090 [49]

Answer:

B. They will conserve energy during reproduction

Explanation:

5 0
2 years ago
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