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Oduvanchick [21]
4 years ago
8

Assume that Na+ is being transported across a membrane via facilitated diffusion. Which of the following conditions would allow

for the most transport of Na+ across that membrane?
Assume that Na+ is being transported across a membrane via facilitated diffusion. Which of the following conditions would allow for the most transport of Na+ across that membrane?
1. Na+ diffusing toward the side of the membrane with K+ and 5% less Na+
2. Na+ diffusing toward the side of the membrane with Cl− and 5% less Na+
3. Na+ diffusing toward the side of the membrane with K+ and 50% less Na+
4. Na+ diffusing toward the side of the membrane with Cl− and 50% less Na+
Chemistry
1 answer:
lesya [120]4 years ago
3 0

Answer:

<h2>4. Na+ diffusing toward the side of the membrane with Cl− and 50% less Na+.</h2>

Explanation:

Facilitated diffusion is a type of transport mechanism in which the special proteins are involved and play an important role in the transport of the atoms, ions or molecules. This mechanism is based on the electrochemical gradient differences. When this difference increase, then the transport of the sodium takes place because sodium ions are chemically attracted by chloride ions. In a facilitated diffusion process, no energy requirement takes place. This process occurs along the concentration gradient.

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According to Boyle's Law,
                                        " the volume of a fixed mass of gas is inversely proportional to the pressure applied on it'.

Mathmatically,
                                    V ∞ 1 / P
Or,
                                    V = k / P
Explanation:
                   The balloon filled with Neon gas outside the chamber will have greater volume than in the chamber because the pressure in the chamber is high as compared to outside. So, the outside force brings the molecule of gas to get closer to each other.
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4 years ago
How many moles of nitrogen gas are in a flask with a volume of 0.25 L at a pressure of 2.96 atm and a temperature of 300 K
aniked [119]

<u>Answer:</u> The number of moles of nitrogen gas is 0.030 moles

<u>Explanation:</u>

To calculate the number of moles of nitrogen, we use the equation given by ideal gas which follows:

PV=nRT

where,

P = pressure of the nitrogen gas = 2.96 atm

V = Volume of the gas = 0.25 L

T = Temperature of the gas = 300 K

R = Gas constant = 0.0821\text{ L. atm }mol^{-1}K^{-1}

n = number of moles of nitrogen gas = ?

Putting values in above equation, we get:

2.96atm\times 0.25L=n\times 0.0821\text{ L. atm }mol^{-1}K^{-1}\times 300K\\\\n=\frac{2.96\times 0.25}{0.0821\times 300}=0.030mol

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6 0
3 years ago
Smaller nuclei are more likely to be stable because:
rjkz [21]

Answer:

B. the strong nuclear force gets counteracted by the presence of neutrons should be the answer.

4 0
2 years ago
The combustion of methane(CH4) produces carbon dioxide and water. Assume that 2.0 mol of CH4 burned in the presence of excess ai
harkovskaia [24]

Answer:

The answer to your question is 98.9 %

Explanation:

Data

moles of methane = CH₄ = 2.0

excess air

Percent yield = ?

mass of CO₂ = 87 g

- Balanced chemical reaction

                CH₄  +  2O₂   ⇒  CO₂  +  2H₂O

      Reactants     Elements       Products

             1                    C                   1

             4                   H                   2

             4                   O                   2

- Calculate the molar mass of CH₄

CH₄ = 12 + 4 = 16 g

- Convert the moles to mass

                     16 g of CH₄ ----------------- 1 mol

                       x                -----------------  2 moles

                       x = (2 x 16) / 1

                       x = 32 g of CH₄

-Calculate the theoretical formation of CO₂

                     16 g of CH₄ ----------------- 44 g of CO₂

                     32 g of CH₄ ----------------  x

                            x = (32 x 44) / 16

                            x = 88 g of CO₂

-Calculate the Percent yield

     Percent yield = Actual yield/Theoretical yield x 100

     Percent yield = 87/88 x 100

    Percent yield = 98.9 %

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