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sladkih [1.3K]
3 years ago
7

Succinate dehydrogenase catalyzes the conversion of succinate to fumarate. The reaction is inhibited by malonic acid, which rese

mbles succinate but cannot be acted upon by succinate dehydrogenase. Increasing the ratio of succinate to malonic acid reduces the inhibitory effect of malonic acid.
Chemistry
1 answer:
koban [17]3 years ago
5 0

Answer:

Succinate is the substrate, and fumarate is the product.

Explanation:

Succinate dehydrogenase is known as an enzyme complex occurs in the inner mitochondrial membrane of the eukaryotes, and many bacterial cells. This is the only enzyme that helps to contribute to both the citric acid cycle and ETC (electron transport chain). In the 6th step of the cycle, SQR utilizes the oxidation of succinate to fumarate and the reduction of ubiquinone to ubiquinol occurs.

This occurs in the inner mitochondrial membrane by pairing the 2 reactions together. Succinate and fumarate only differ in their geometrical structure around their double bond, and the other contains a trans double bond.

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2 years ago
Name the alkanes please help
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4 0
2 years ago
A mixture of CuSO4 · 5H2O and MgSO4 · 7H2O is heated until all the water is lost. If 5.127 g of the mixture gives 2.817 g of the
Nadusha1986 [10]

Answer:

Let the mixture is X% by mass of CuSO

4

.5H

2

O and 100 - X % by mass of MgSO

4

.7H

2

O. 5.0 g of mixture will contain 0.05X g CuSO

4

.5H

2

O and 5.0 - 0.05X g MgSO

4

.7H

2

O

The molar masses of CuSO

4

.5H

2

O and MgSO

4

.7H

2

O are 249.7 g/mol and 246.5 g/mol respectively.

The number of moles of CuSO

4

.5H

2

O=

249.7

0.05X

=2.00×10

−4

X moles.

Explanation:

Pls mark it as branliest answere thanks

3 0
2 years ago
In acid solution, water can add to the double bond of 2-butenedioic acid to form 2-hydroxysuccinic acid.
satela [25.4K]
So, what is the question?
6 0
2 years ago
Determine the rate law, including the values of the orders and rate law constant, for the following reaction using the experimen
olga55 [171]

Answer: Rate law=k[A]^1[B]^2, order with respect to A is 1, order with respect to B is 2 and total order is 3. Rate law constant is 3L^2mol^{-2}s^{-1}

Explanation: Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

Rate=k[A]^x[B]^y

k= rate constant

x = order with respect to A

y = order with respect to A

n = x+y = Total order

a) From trial 1: 1.2\times 10^{-2}=k[0.10]^x[0.20]^y    (1)

From trial 2: 4.8\times 10^{-2}=k[0.10]^x[0.40]^y    (2)

Dividing 2 by 1 :\frac{4.8\times 10^{-2}}{1.2\times 10^{-2}}=\frac{k[0.10]^x[0.40]^y}{k[0.10]^x[0.20]^y}

4=2^y,2^2=2^y therefore y=2.

b) From trial 2: 4.8\times 10^{-2}=k[0.10]^x[0.40]^y    (3)

From trial 3: 9.6\times 10^{-2}=k[0.20]^x[0.40]^y   (4)

Dividing 4 by 3:\frac{9.6\times 10^{-2}}{4.8\times 10^{-2}}=\frac{k[0.20]^x[0.40]^y}{k[0.10]^x[0.40]^y}

2=2^x,2=2^1, x=1

Thus rate law is Rate=k[A]^1[B]^2

Thus order with respect to A is 1 , order with respect to B is 2 and total order is 1+2=3.

c) For calculating k:

Using trial 1:  1.2\times 10^{-2}=k[0.10]^1[0.20]^2

k=3 L^2mol^{-2}s^{-1}.



6 0
3 years ago
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