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serious [3.7K]
3 years ago
12

g Consider a uniport system where a carrier protein transports an uncharged substance A across a cell membrane. Suppose that at

a certain ratio of [ A ] inside to [ A ] outside , the Δ G for the transport of substance A from outside the cell to the inside, A outside → A inside , is − 14.1 kJ/mol at 25°C. What is the ratio of the concentration of substance A inside the cell to the concentration outside?
Chemistry
1 answer:
Alborosie3 years ago
3 0

Answer :  The ratio of the concentration of substance A inside the cell to the concentration outside is, 296.2

Explanation :

The relation between the equilibrium constant and standard Gibbs free energy is:

\Delta G^o=-RT\times \ln Q\\\\\Delta G^o=-RT\times \ln (\frac{[A]_{inside}}{[A]_{outside}})

where,

\Delta G^o = standard Gibbs free energy  = -14.1 kJ/mol

R = gas constant = 8.314 J/K.mol

T = temperature = 25^oC=273+25=298K

Q  = reaction quotient

[A]_{inside} = concentration inside the cell

[A]_{outside} = concentration outside the cell

Now put all the given values in the above formula, we get:

-14.1\times 10^3J/mol =-(8.314J/K.mol)\times (298K)\times \ln (\frac{[A]_{inside}}{[A]_{outside}})

\frac{[A]_{inside}}{[A]_{outside}}=296.2

Thus, the ratio of the concentration of substance A inside the cell to the concentration outside is, 296.2

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How many grams are in 6.8L of Oxygen gas (O2) at STP
zubka84 [21]

Answer:

9.7 g

Explanation:

From the question,

Note: The molar volume of all gas at stp is 22.4 dm³ or 22.4 L

1 mol of  oxygen gas (O₂) at stp = 22.4 dm³

X mole of oxygen gas (O₂) at stp = 6.8 L

X = (1 mol×6.8 L)/22.4 L

X = 0.3036 mol.

But,

Number of mole (n) = mass (m)/molar mass (m')

n = m/m'

m = n×m'.................. Equation 2

Where n = 0.3036 mol, m' = 32 g/mol

Substitute into equation 2

m = 0.3036×32

m = 9.7 g

4 0
2 years ago
In the molecule SF4, sulfur makes four covalent bonds. Therefore, four of its six valence electrons need to be unpaired. The orb
Bezzdna [24]

Explanation:

As it is given that there are six electrons with four of them unpaired in the degenerate orbital.

As in a p-orbital there are only 3 sub-orbitals, that is, p_{x}, p_{y}, and p_{z}. In these sub-orbitals, a maximum of 6 electrons can be accommodated.

Th next higher orbital is d-orbital which can contain a maximum of 10 electrons. There are 5 degenerate orbitals present in a d-orbital.

So, a d-orbital can easily accommodate six electrons with four of them unpaired.

Thus, we can conclude that 5 degenerate orbitals are needed to contain six electrons with four of them unpaired.

3 0
3 years ago
When 4.31 g of a nonelectrolyte solute is dissolved in water to make 635 mL of solution at 28 °C, the solution exerts an osmotic
blondinia [14]

Answer:

Molar concentration is 0.050 M

Explanation:

Osmotic pressure -

Osmotic pressure is pressure applied  to stop the flow of solvent across a semipermeable membrane, from its high concentration to  its low concentration , it is a type of colligative property , i.e. , it depends on the number of moles of solute.

Osmotic pressure can be calculated from the formula -

π = CRT

π = Osmotic pressure ( in atm )

C = molarity of the solution

R = universal gas constant ( 0.082 L.atm / K.mol )

T = temperature ( Kelvin )

From the question ,

π = 945 torr

since,

760 torr = 1 atm

1 torr = 1 / 760 atm

945 torr = 1 / 760 * 945 atm

945 torr = 1.24 atm

Temperature = T = 28°C

(adding 273 To °C to convert it to K)

T = 28 + 273 = 301 K

Using the equation of osmotic pressure,

π = CRT

C = π / RT

putting the

C = 1.24 atm / 0.082 L.atm / K.mol * 301 K

C = 1.24 / 24.68

C = 0.050 M

Hence,

The Molar concentration is 0.050 M.  

3 0
3 years ago
Calculate the heat in kJ required to convert 2.1 g of water at 52.1°C to steam at 100°C. The specific heat of water is 4.184 J/g
kondaur [170]

Answer:

5.167 kJ

Explanation:

We have to divide the heating process into two steps: one for the heating process of liquid water (1) and the other for the phase transition from liquid water to steam at 100°C (2)

1 - heating from 52.1°C to 100°C:

heat(1) = m x Cp x ΔT = 2.1 g x 4.184 J/g°C x (100°C-52.1°C) = 420.9 J

2 - vaporization at 100°C:

heat(2) = m x ΔHv = 2.1 g x 2260 J/g = 4746 J

Finally, we add the heat values of the steps:

heat required = heat(1) + heat(2) = 420.9 J + 4746 J = 5166.9 J

Since 1 kJ= 1000 J, we convert from J to kJ:

5166.9 J x 1 kJ/1000 J = 5.1669 kJ ≅ 5.167 kJ

4 0
3 years ago
What volume of a 6.0m hcl solution is required to make 250.0 milliters of 1.5 m hcl
Georgia [21]

Answer : The volume for 6.0m HCl solution required = 62.5 ml

Solution : Given,

Initial concentration of HCl solution = 6.0m

Final concentration of HCl solution = 1.5m

Final volume of HCl solution = 250 ml

Initial volume of HCl solution = ?

Formula used for dilution is,

M_1V_1=M_2V_2

where,

M_1 = initial concentration

M_2 = final concentration

V_1 = initial volume

V_2 = final volume

Now put all the given values in above formula, we get the initial volume of HCl solution.

6.0m\times V_1=1.5m\times 250ml

V_1 = 62.5 ml

Therefore, the volume for 6.0m HCl solution required = 62.5 ml


8 0
3 years ago
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