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4 years ago

13

when an individual goes without eating for a day, his or her blood sugar remains about the same throughout the day this relative

ly constant condition is maintained by

1 answer:

Len [333]4 years ago

5 0

The answer is homeostatic control

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The atmosphere of the planet Mars is 95.3% carbon dioxide, 2.6% nitrogen, 1.9% argon, with the remaining fraction being traces o

kodGreya [7K]

Answer:

Mean Partial pressure of Nitrogen in Mars' atmosphere = 15.86 Pa

Explanation:

According to Dalton's law of Partial Pressure, the total pressure exerted by a mixture of ideal gases (that do not react together) is the sum of the partial pressures of the individual gases that make up the mixture. It goes further to explain that the partial pressure of a gas in a mixture of gases is equal to its mole fraction of that gas multipled by the total pressure exerted by the mixture of gases.

Total Pressure exerted by the mixture of gases in the atmosphere on Mars = Mean atmospheric pressure on Mars = 610 Pa

Partial pressure of Nitrogen = (mole fraction or mole percentage of Nitrogen in the atmosphere) × (total pressure exerted by all the gases in the atmosphere)

Mole percentage of Nitrogen in the atmosphere of Mars = 2.6%

Partial pressure of Nitrogen = 2.6% × 610 = 15.86 Pa

Mean Partial pressure of Nitrogen in Mars' atmosphere = 15.86 Pa

Hope this Helps!!!

3 0

3 years ago

Compare and contrast the movement of electric charge in a solution with the transfer of electric charge between solid objects

Kamila [148]

The idea of electric field was presented by Michael Faraday. The electrical field constrain acts between two charges, similarly that the gravitational field compel acts between two masses.

6 0

4 years ago

The answer to question 2

Bad White [126]

Answer:

12

Explanation:

You will need a chemical equation with masses and molar masses, so let’s gather all the information in one place.

$M_{r}$ : 258.21 18.02

KAl(SO₄)₂·xH₂O ⟶ KAl(SO₄)₂ + xH₂O

Mass/g: 4.74 2.16

Step 1. Calculate the mass of the KAl(SO₄)₂.

Mass = 4.74 g – 2.16 g = 2.58 g.

Step 2. Calculate the moles of each product.

$\text{Moles of KAl(SO}_{4})_{2} = \text{2.58 g} \times \frac{\text{1 mol} }{\text{258.21 g}} = 9.992 \times 10^{-3} \text{ mol}$

$\text{Moles of H}_{2}\text{O} = \text{2.16 g} \times \frac{\text{1 mol} }{\text{18.02 g}} = \text{ 0.1200 mol}$

Step 3. Calculate the molar ratio of the two products.

$\frac{\text{Moles of KAl(SO}_{4})_{2}}{\text{Moles of H}_{2}\text{O}} = \frac{ 9.992 \times 10^{-3} \text{ mol}}{\text{ 0.1200 mol} } = \frac{1 }{12.01} \approx \frac{ 1}{ 12}$

1 mol of KAl(SO₄)₂ combines with 12 mol H₂O, so x = 12.

3 0

3 years ago

Diphosphorus pentoxide(P2O5) reacts with water to form phosphoric acid, a major industrial acid. In the laboratory, the oxide is

Akimi4 [234]

Answer: The mass of $4.65\times 10^{22}$ molecules of phosphorus pentoxide is 20.5 g

Explanation:

According to avogadro's law, 1 mole of every substance weighs equal to the molecular mass and contains avogadro's number $6.023\times 10^{23}$ of particles.

To calculate the moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given molecules}}{\text {avogadro's number}}=\frac{4.65\times 10^{22}}{6.023\times 10^{23}}=0.0772moles$

1 mole of $P_2O_5$ weigh = 283.9 g

Thus 0.0772 moles of $P_2O_5$ weigh = $\frac{283.9}{1}\times 0.0722=20.5g$

Thus the mass of $4.65\times 10^{22}$ molecules of phosphorus pentoxide is 20.5 g

3 0

3 years ago

Gases do not settle at the bottom of the vessel why

bulgar [2K]

Explanation:

Gases are very less denser also, they've negligible intermolecular force of attraction between the particles of the gas. So, they all are free to roam seperately and hence making a negligible volume for which they become heavy settle down.

7 0

3 years ago