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natta225 [31]
2 years ago
9

QUICK PLEASE

Chemistry
1 answer:
masya89 [10]2 years ago
3 0

Answer:

20.0% w/v A

Explanation:

A 20.0 w/V...

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Where in the lungs does gas exchange occur
Lina20 [59]

Answer: Between the alveoli and a network of tiny blood vessels called capillaries, which are located in the walls of the alveoli.

7 0
3 years ago
(Can someone please help me...im literally done with brainly...) Which answer best completes the following sentence? _____ is an
Furkat [3]

Answer:

(1) breaking a pencil (2) rusting of iron

Explanation:

breaking a pencil does not alter the chemical properties of the pencil, it merely breaks it into 2 while the rusting of iron is changing the properties chemically because the iron is oxidizing and reacting with the water and oxygen in the atmosphere

5 0
3 years ago
Consider the following reaction at 25 °C: 4Fe(s) + 3O2(g) ⇌ 2Fe2O3(s) An equilibrium mixture contains 1.0 mol Fe, 1.0 × 10–3 mol
tino4ka555 [31]

Answer:

Kc = Kc = 8.0 * 10^9

Kp = 5.5 *10^5

Explanation:

Step 1: Data given

Temperature = 25.0 °C

Number of moles Fe = 1.0 moles

Number of moles O2 = 1.0 * 10^-3 moles

Number of moles Fe2O3 = 2.0 moles

Volume = 2.0 L

Step 2: The balanced equation

4Fe(s) + 3O2(g) ⇌ 2Fe2O3(s)

Step 3: Calculate molarity

Molarity = moles / volume

[Fe] = 1.0 moles / 2.0 L

[Fe] = 0.5 M

[O2] = 0.001 moles / 2.0 L

[O2] = 0.0005 M

[Fe2O3] = 2.0 moles / 2.0 L

[Fe2O3] = 1.0 M

Step 4: Calculate Kc

Kc =1/ [O2]³

Kc = 1/0,.000000000125

Kc = 8.0 * 10^9

Step 5: Calculate Kp

Kp = Kc*(R*T)^Δn

⇒with Kc = 8.0*10^9

⇒with R = 0.08206 L*atm /mol*K

⇒with T = 298 K

⇒with Δn = -3

Kp = 8.10^9 *(0.08206 * 298)^-3

Kp = 5.5 *10^5

4 0
2 years ago
You want to mix 1 molar Nitric acid with water to dilute the nitric acid to .5 molar how should you mix these two liquids togeth
navik [9.2K]

Answer:

Freeze the water

Explanation:

5 0
2 years ago
1. Take the reaction: NH3 + O2 + NO + H2O. In an experiment, 3.25g of NH3 are allowed
Rudiy27

Answer:

5.74g of NO

Explanation:

Step 1:

The balanced equation for the reaction. This is given below:

4NH3 + 5O2 —> 4NO + 6H2O

Step 2:

Determination of the masses of NH3 and O2 that reacted and the mass of NO produced from the balanced equation. This is illustrated below:

Molar Mass of NH3 = 14 + (3x1) = 14 + 3 = 17g/mol

Mass of NH3 from the balanced equation = 4 x 17 = 68g

Molar Mass of O2 = 16x2 = 32g/mol

Mass of O2 from the balanced equation = 5 x 32 = 160g

Molar Mass of NO = 14 + 16 = 30g/mol

Mass of NO from the balanced equation = 4 x 30 = 120g

From the balanced equation above,

68g of NH3 reacted with 160g of O2 to produce 120g of NO.

Step 3:

Determination of the limiting reactant.

We need to determine the limiting because it will be used to calculate the maximum yield of the reaction. This is illustrated below:

From the balanced equation above,

68g of NH3 reacted with 160g of O2.

Therefore, 3.25g of NH3 will react with = (3.25 x 160)/68 = 7.65g of O2.

From the simple illustration above, we can see that lesser mass of O2 is needed to react with 3.25g of NH3. Therefore, NH3 is the limiting reactant while O2 is the excess reactant.

Step 4:

Determination of the mass of NO produced from the reaction.

In this case the limiting reactant will be used because all of it were used in the reaction.

The limiting reactant is NH3.

From the balanced equation above,

68g of NH3 reacted to produce 120g of NO.

Therefore, 3.25g of NH3 will react to produce = (3.25 x 120)/68 = 5.74g of NO.

From the calculations made above, 5.74g of NO is produced.

4 0
3 years ago
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