____is used as anode for prevention of corrosion 1 aluminium 2 magnesium 3 iron

25. Which is not a form of chemical changer

Salsk061 [2.6K]

Answer:

C. Digestion is the answer.

6 0

2 years ago

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A 25.00 ml solution of sulfuric acid H2SO4 is titrated to phenolphthalein end point with 27.00 ml of 1.700 M KOH

Nastasia [14]

<h3>Answer:</h3>

0.918 M

<h3>Explanation:</h3>

Assuming the question requires we calculate the Molarity of sulfuric acid:

We are given:

Volume of the acid, H₂SO₄ = 25.00 ml
Volume of the base, KOH = 27.00 mL
Molarity of the base, KOH is 1.70 M

We can calculate the molarity of the acid using the following steps;

<h3>Step 1: Write the chemical equation for the reaction.</h3>

The reaction is an example of a neutralization reaction where a base reacts with an acid to form salt and water.

Therefore, the balanced equation will be;

H₂SO₄(aq) + 2KOH(aq) → K₂SO₄(aq) + 2H₂O(l)

<h3>Step 2: Determine the moles of the base, KOH </h3>

When given molarity and the volume of a solution, the number of moles can be calculated by multiplying molarity with volume.

Number of moles = Molarity × Volume

= 1.700 M × 0.027 L

= 0.0459 moles

Thus, moles of KOH used is 0.0459 moles

<h3>Step 3: Determine the number of moles of the Acid, H₂SO₄</h3>

From the reaction, 1 mole of the acid reacts with 2 moles of KOH

Therefore, the mole ratio of H₂SO₄ to KOH is 1 : 2

Thus, moles of H₂SO₄ = Moles of KOH ÷ 2

= 0.0459 moles ÷ 2

= 0.02295 moles

<h3>Step 4: Calculate the molarity of the Acid </h3>

Molarity is the concentration of a solution in moles per liter

Molarity = Moles ÷ Volume

Molarity of the acid = 0.02295 moles ÷ 0.025 L

= 0.918 M

Thus, the molarity of the acid, H₂SO₄ is 0.918 M

5 0

3 years ago

Antimony has two naturally occuring isotopes, 121 Sb and 123 Sb . 121 Sb has an atomic mass of 120.9038 u , and 123 Sb has an at

valina [46]

Answer:

Percentage abundance of 121 Sb is = 57.2 %

Percentage abundance of 123 Sb is = 42.8 %

Explanation:

The formula for the calculation of the average atomic mass is:

$Average\ atomic\ mass=(\frac {\%\ of\ the\ first\ isotope}{100}\times {Mass\ of\ the\ first\ isotope})+(\frac {\%\ of\ the\ second\ isotope}{100}\times {Mass\ of\ the\ second\ isotope})$

Given that:

Since the element has only 2 isotopes, so the let the percentage of first be x and the second is 100 -x.

For first isotope, 121 Sb :

% = x %

Mass = 120.9038 u

For second isotope, 123 Sb:

% = 100 - x

Mass = 122.9042 u

Given, Average Mass = 121.7601 u

Thus,

$121.7601=\frac{x}{100}\times 120.9038+\frac{100-x}{100}\times 122.9042$

$120.9038x+122.9042\left(100-x\right)=12176.01$

Solving for x, we get that:

x = 57.2 %

<u>Thus, percentage abundance of 121 Sb is = 57.2 % </u>

<u>percentage abundance of 123 Sb is = 100 - 57.2 % = 42.8 %</u>

6 0

3 years ago

the reaction of Al with HCl to produce hydrogen gas. What is the pressure of H2 if the hydrogen gas collected occupies 14 L at 3

juin [17]

Answer:

Pressure for H₂ = 11.9 atm

Option 5.

Explanation:

We determine the complete reaction:

2Al(s) + 6HCl(aq) → 2AlCl₃(aq) + 3H₂(g)

As we do not know anything about the HCl, we assume that the limiting reactant is the Al and the acid is the excess reagent.

Ratio is 2:3.

2 moles of Al, can produce 3 moles of hydrogen

Therefore 4.5 moles of Al must produce (4.5 . 3) / 2 = 6.75 moles

Now we can apply the Ideal Gases law to find the H₂'s pressure

P . V = n . R . T → P = (n . R .T) / V

We replace data: (6.75 mol . 0.082L.atm/mol.K . 300K) / 14L

Pressure for H₂ = 11.9 atm

6 0

2 years ago

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What would increase the amount of your carbon dioxide output?

SSSSS [86.1K]

Answer:

Consuming electricity: Burning fossil fuels emits CO2, with coal releasing twice as much of the gas as petroleum. Worldwide, fossil fuels generate 85 percent of electricity. The number of coal-burning plants will increase as China and India continue to industrialize.

4 0

3 years ago