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3 years ago

Which of the following forms of oxygen can undergo disproportionation?

1 answer:

5 0

<span>disproportionation is a type of redox reaction in which an element can undergo both oxidation and reduction.

Let's take a look at the choices:
First we have the oxide ion. Oxide ion has a charge of -2 which is the lowest charge that an oxygen atom can have. Therefore, an oxide ion cannot be further reduced, so this choice is not correct.
Next we have the peroxide ion. The oxygen has a charge of -1 which means it can be further reduced. So, this choice is acceptable
Last but not least, we have the superoxide ion. The oxygen has a charge of -1/2 which means it can be further reduced. So, this choice is also acceptable.

Based on this, we have two accepted choices which are b and c.</span>

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B.the amount of energy transferred.

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3 years ago

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Given the balanced equation:

Monica [59]

Answer: 7.88375g

Explanation:

Here is the dimensional analysis table

7g O2 | 1 mol O2 | 2 mol H2O | 18.02 g H2O

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You use grams to convert to moles of O2, then use that to find grams of H20

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3 years ago

A slice of Swiss cheese contains 41 mg of sodium.

larisa86 [58]

Answer:

a. 41 mg equals 0.041 grams.

b. 41 mg equals 0.0014462 ounces

c. 41 mg equals 9.039*10⁻⁵ pounds

Explanation:

You know that a slice of Swiss cheese contains 41 mg of sodium.

a. What is this mass in grams?

Knowing that 1 mg = 10⁻³ g, you can apply the following rule of three: if 1 mg equals 10⁻³ g or 0.001 grams, 41 mg will be equivalent to how much mass in g?

$mass=\frac{41 mg*0.001 g}{1 mg}$

mass= 0.041 grams

<u><em> 41 mg equals 0.041 grams.</em></u>

b. What is this mass in ounces?

Knowing that 1 mg = 3.5274 * 10⁻⁵ ounces, you can apply the following rule of three: if 1 mg equals 3.5274 * 10⁻⁵ ounces, 41 mg will be equivalent to how much mass in ounces?

$mass=\frac{41 mg*3.5274*10^{-5}ounces }{1 mg}$

mass= 1.4462*10 ⁻³ ounces= 0.0014462 ounces

<u><em>41 mg equals 0.0014462 ounces</em></u>

c. What is this mass in pounds?

Knowing that 1 mg = 2.20462 * 10⁻⁶ pounds, you can apply the following rule of three: if 1 mg equals 2.20462 * 10⁻⁶ pounds, 41 mg will be equivalent to how much mass in pounds?

$mass=\frac{41 mg*2.20462*10^{-6}pounds }{1 mg}$

mass= 9.039*10⁻⁵ pounds

<u><em>41 mg equals 9.039*10⁻⁵ pounds</em></u>

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3 years ago

For the following reaction, 6.94 grams of water are mixed with excess sulfur dioxide . Assume that the percent yield of sulfurou

Alexxx [7]

<h3>Answer:</h3>

#a. Theoretical yield = 31.6 g

#b. Actual yield = 25.72 g

<h3>Explanation:</h3>

The equation for the reaction between sulfur dioxide and water to form sulfurous acid is given by the equation;

SO₂(g) + H₂O(l) → H₂SO₃(aq)

The percent yield of H₂SO₃ is 81.4%

Mass of water that reacted is 6.94 g

#a. To get the theoretical yield of H₂SO₃ we need to follow the following steps

Step 1: Calculate the moles of water

Molar mass of water = 18.02 g/mol

Mass of water = 6.94 g

But, moles = Mass/molar mass

Moles of water = 6.94 g ÷ 18.02 g/mol

= 0.385 mol

Step 2: Calculate moles of H₂SO₃

From the equation, the mole ratio of water to H₂SO₃ is 1 : 1

Therefore, moles of water = moles of H₂SO₃

Hence, moles of H₂SO₃ = 0.385 mol

Step 3: Theoretical mass of H₂SO₃

Mass = moles × Molar mass

Molar mass of H₂SO₃ = 82.08 g/mol

Number of moles of H₂SO₃ = 0.385 mol

Therefore;

Theoretical mass of H₂SO₃ = 0.385 mol × 82.08 g/mol

= 31.60 g

Thus, the theoretical yield of H₂SO₃ is 31.6 g

<h3>#b. Calculating the actual yield</h3>

We need to calculate the actual yield

Percent yield of H₂SO₃ is 81.4%

Theoretical yield is 31.60 g

But; Percent yield = (Actual yield/theoretical yield)×100

Therefore;

Actual yield = Percent yield × theoretical yield)÷ 100

= (81.4 % × 31.6) ÷ 100

= 25.72 g

The percent yield of H₂SO₃ is 25.72 g

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3 years ago

What is the correct name for this formula: BaCl2

Inessa05 [86]

BaCI2 stands for Barium Chloride. Hope this helps!

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3 years ago

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