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motikmotik
3 years ago
6

Help, please I don't understand what I have to do

Chemistry
1 answer:
8_murik_8 [283]3 years ago
4 0

Answer:

Is there a picture To go with this?

Explanation:

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Which carbon atom(s) of pyruvate is(are) first converted to carbon dioxide by pyruvate dehydrogenase complex?
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The carbon atom(s) of pyruvate is(are) first converted to carbon dioxide by pyruvate dehydrogenase complex is the second number of carbon of pyruvate goes to oxidation and convert it to CO2 in Krebs cycle.

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Krebs cycle is also known as citric acid cycle it is the conversion of sugar to the direct energy in the form of ATP which further goes to mitochondria as it is the power house of the human cell.

Pyruvate molecule release second number carbon from the chain and undergoes oxidation to form the CO2.

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2 years ago
Which statements are true in regard to the VSEPR theory?
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How many grams of glucose are in 4.5x1023 molecules of glucose?:
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3 years ago
The bonds that link many water molecules together to form a water drop are _____ bonds.
Gelneren [198K]

The bonds found between water molecules are called:

Hydrogen bonds

which contribute to water having a high number of Van Der Waals forces.

Explanation:

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7 0
3 years ago
An ideal gas is brought through an isothermal compression process. The 3.00 mol of gas goes from an initial volume of 261.6×10−6
Eduardwww [97]

Answer : The temperature and the final pressure of the gas is, 586.83 K and 1.046\times 10^{9}atm respectively.

Explanation : Given,

Initial volume of gas = 261.6\times 10^{-6}m^3

Final volume of the gas = 138.2\times 10^{-6}m^3

Heat released = -9340 J

First we have to calculate the temperature of the gas.

According to the question, this is the case of isothermal reversible compression of gas.

As per first law of thermodynamic,

\Delta U=q+w

where,

\Delta U = internal energy

q = heat

w = work done

As we know that, the term internal energy is the depend on the temperature and the process is isothermal that means at constant temperature.

So, at constant temperature the internal energy is equal to zero.

q=-w

Thus, w = -q = 9340 J

The expression used for work done will be,

w=nRT\ln (\frac{V_2}{V_1})

where,

w = work done = 9340 J

n = number of moles of gas  = 3 mole

R = gas constant = 8.314 J/mole K

T = temperature of gas  = ?

V_1 = initial volume of gas

V_2 = final volume of gas

Now put all the given values in the above formula, we get the temperature of the gas.

9340J=3mole\times 8.314J/moleK\times T\times \ln (\frac{261.6\times 10^{-6}m^3}{138.2\times 10^{-6}m^3})

T=586.83K

Now we have to calculate the final pressure of the gas by using ideal gas equation.

PV=nRT

where,

P = final pressure of gas = ?

V = final volume of gas = 138.2\times 10^{-6}m^3=138.2\times 10^{-9}L

T = temperature of gas = 586.83 K

n = number of moles of gas = 3 mole

R = gas constant = 0.0821 L.atm/mole.K

Now put all the given values in the ideal gas equation, we get:

P\times (138.2\times 10^{-9}L)=3mole\times (0.0821L.atm/mole.K)\times (586.83K)

P=1.046\times 10^{9}atm

Therefore, the temperature and the final pressure of the gas is, 586.83 K and 1.046\times 10^{9}atm respectively.

6 0
3 years ago
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