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3 years ago

How many phosphate bonds are responsible for the high energy content of ATP?

Chemistry

2 answers:

liraira [26]3 years ago

8 0

Answer:

A one

Explanation:

edge test

Nataly_w [17]3 years ago

4 0

The answer is a. one. There are three phosphate bonds in the ATP but only the first bond is responsible for the high energy. When this bond break, ATP will change to ADP.

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Match the factors which affect the rate of dissolving/dissociation/diffusion.

aev [14]

Answer:

Increased surface area - finely divided solute

like dissolves like - matching polarity

temperature - rate proportional to kinetic energy

stirring spreads - solute throughout solution

4 0

3 years ago

Question 1 (1 point)

andrezito [222]

Answer:

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Explanation:

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5 0

3 years ago

Which equation best represents the behavior of acetic acid, hc2h3o2, in water?

frutty [35]

The equation that best represents the behavior of acetic acid in water is; CH3CO2H + H2O ⇄ CH3CO2− + H3O+.

Acetic acid, like all other acids dissociates in water. The equation for the dissociation of acetic acid in water is; CH3CO2H + H2O ⇄ CH3CO2− + H3O+.

During this dissociation, the acid proton in acetic acid is transferred to water to form the oxonium ion H3O+.

The presence of H3O+ in solution accounts for all the observed properties of acetic acid in solution.

Learn more: brainly.com/question/14072179

3 0

2 years ago

How many moles of pcl5 can be produced from 23.0 g of p4 (and excess cl2)? express your answer to three significant figures and

NeX [460]

Balance Chemical equation is,

P₄ + 10 Cl₂ → 4 PCl₅

According to Balance Equation,

123.89 g (1 mole) of P₄ reacts to produce = 4 Moles of PCl₅
Then,
23 g of P₄ will react with excess Cl₂ to produce = X moles of PCl₅

Solving for X,
X = (4 mol × 23 g) ÷ 123.89 g

X = 0.742 g of PCl₅
Result:
When 23 g of P₄ is reacted with excess Cl₂, 0.742 g of PCl₅ is produced.

4 0

4 years ago

Buffer preparation. You wish to prepare a buffer consisting of acetic acid and sodium acetate with a total acetic acid plus acet

Hoochie [10]

Answer:

0.182 moles of acetic acid are needed, this means 10.93 g.

0.318 moles of sodium acetate are needed, this means 26.08 g.

Explanation:

The Henderson–Hasselbalch (H-H) equation tells us the relationship between the concentration of an acid, its conjugate base, and the pH of a buffer:

pH = pka + $log\frac{[A^{-} ]}{[HA]}$

In this case, [A⁻] is the concentration of sodium acetate, and [HA] is the concentration of acetic acid. The pka is a value that can be looked up in literature: 4.76.

From the problem we know that

[A⁻] + [HA] = 250 mM = 0.250 M eq. 1

We use the H-H equation, using the data we know, to describe [A⁻] in terms of [HA]:

5.0 = 4.76 + $log\frac{[A^{-} ]}{[HA]}$

$0.24=log\frac{[A^{-} ]}{[HA]}\\\\10^{0.24}=\frac{[A^{-} ]}{[HA]}\\ 1.74 [HA] = [A^{-}]$ eq.2

Now we replace the value of [A⁻] in eq. 1, to calculate [HA]:

1.74 [HA] + [HA] = 0.250 M

[HA] = 0.091 M

Then we calculate [A⁻]:

[A⁻] + 0.091 M = 0.250 M

[A⁻] = 0.159 M

Using the volume, we can calculate the moles of each substance:

moles of acetic acid = 0.091 M * 2 L = 0.182 moles
moles of sodium acetate = 0.159 M * 2 L = 0.318 moles

Using the molecular weight, we can calculate the grams of each substance:

grams of acetic acid = 0.182 mol * 60.05 g/mol = 10.93 g
grams of sodium acetate = 0.318 mol * 82.03 g/mol = 26.08 g

8 0

3 years ago