Molecular compounds result from covalent bonding which are called _______.This is for high school physical science

Answer:

(C3H8) produces 660 g of CO2 and 360 g of H2O

Explanation:

The balanced chemical equation for the combustion of propane (C3H8) is:

C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)

This equation tells us that for every molecule of propane (C3H8) that reacts with 5 molecules of oxygen (O2), 3 molecules of carbon dioxide (CO2) and 4 molecules of water (H2O) are produced.

So, if we have 220. g of propane (C3H8), we can find the amount of CO2 and H2O produced by using the mole ratio from the balanced equation:

1 mole C3H8 reacts with 5 moles of O2 to produce 3 moles of CO2 and 4 moles of H2O

We can find the number of moles of C3H8 by dividing the mass by the molar mass of C3H8 (44 g/mol):

220 g / 44 g/mol = 5 moles C3H8

So, the number of moles of CO2 and H2O produced can be found by multiplying the number of moles of C3H8 by the mole ratio:

3 moles CO2 = 3 moles CO2/1 mole C3H8 * 5 moles C3H8 = 15 moles CO2

4 moles H2O = 4 moles H2O/1 mole C3H8 * 5 moles C3H8 = 20 moles H2O

Finally, we can convert the number of moles of CO2 and H2O to grams by multiplying by their molar masses (44 g/mol for CO2 and 18 g/mol for H2O):

15 moles CO2 * 44 g/mol = 660 g CO2

20 moles H2O * 18 g/mol = 360 g H2O

So, the combustion of 220 g of propane (C3H8) produces 660 g of CO2 and 360 g of H2O.

Answer:

Henderson Hasselbalch equation: pH = pKa + log [salt]/[acid]

You need to know the pKa for acetic acid. Looking it up one finds it to be 4.76

(a). pH = 4.76 + log [0.13]/[0.10]

= 4.76 + 0.11

= 4.87

(b) KOH + CH3COOH =>H2O + CH3COOK so (acid)goes down and (salt)goes up. Assuming no change in volume, you have 0.10 mol acid - 0.02 mol = 0.08 mol acid and 0.13 mol salt + 0.02 mol = 0.15 mol salt

pH = 4.76 + log [0.15]/[0.08]

= 4.76 + 0.27

= 5.03

Final answer:

The pH of the buffer with 0.11 mol acetic acid and 0.13 mol sodium acetate in 1.00 L is 4.91, calculated using the Henderson-Hasselbalch equation. The second part of the question regarding the pH change after the addition of '2' is unanswerable without further information on what is being added.

Explanation:

To answer the question of what the pH of the buffer solution containing 0.11 mol of acetic acid and 0.13 mol of sodium acetate in 1.00 L is, we can apply the Henderson-Hasselbalch equation:

pH = pKa + log([A-]/[HA])

Where [A-] is the concentration of the acetate ion and [HA] is the concentration of acetic acid. For acetic acid, the pKa is approximately 4.76. Since we have 0.11 mol of acetic acid and 0.13 mol of sodium acetate in 1.00 L solution, the concentrations are 0.11 M and 0.13 M respectively.

Substituting these values into the Henderson-Hasselbalch equation gives:

pH = 4.76 + log(0.13/0.11)

Calculating the log(0.13/0.11) yields approximately 0.15. Therefore:

pH = 4.76 + 0.15 = 4.91

The question "What is the pH of the buffer after the addition of 2?" seems to be incomplete, as it does not specify what '2' refers to. If '2' refers to adding 2 moles of a strong acid or base, for instance, the pH would change significantly and the buffer capacity might be exceeded. The exact effect on pH would depend on the nature of the substance added (acid or base) and its quantity. Without specifics, this part of the question cannot be accurately answered.

The concept of buffer capacity is relevant to discuss here. Buffer capacity refers to the amount of acid or base a buffer can absorb without a significant change in pH. Buffer solutions with higher molar concentrations of both the acid and the corresponding salt will have greater buffer capacity.

Learn more about Buffer Solution pH here:

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Answer:

Moles = 0.375

Explanation:

Moles= m/M

= 12/32 = 0.375mol

Answer:

b and c

Explanation:

the problem was solved through the experiment and tested

Answer:

A

Explanation:

Halogens have 7 electrons in their valence shell and requires just one electron to achieve their stable structure. Because of this they have high electron affinity and hence high electronegativity and they are strong oxidizing agents. Oxidation is the loss of electrons . Halogens have a high readiness to take electrons which a metal loses thereby oxidizing it. The other options are wrong as they involve compounds and not the elemental form as stated in the question.

The specie which is acting as a catalyst is; Ag+(aq).

Discussion:

The catalyst is a specie that exists in the same form at the beginning and end of the reaction.

The reaction's mechanism is as follows;

• Step 1: Ag+(aq) + Ce⁴+(aq) <-----> Ag²+(aq) + Ce³+(aq)

• Step 2: Tl+(aq) + Ag²+(aq) -----> Tl²+(aq) + Ag+(aq)

• Step 3: Tl²+(aq) + Ce⁴+(aq) -----> Tl³+(aq) + Ce³+(aq)

Evidently, although Ag+(aq) was converted to Ag²+(aq) in Step 1 of the reaction; the Ag²+(aq) is reverted back to Ag+(aq) in Step 2 of the reaction.

Read more:

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Answer:

Ag⁺ acts as the catalyst.

Explanation:

Hello,

In this case, each step is reorganized:

- Step 1:

- Step 2:

- Step 3:

In such a way, Ag⁺ is converted to Ag²⁺ in the first step, but then it is regenerated to simple Ag⁺, therefore, Ag⁺ acts as the catalyst.

Best regards.