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mrs_skeptik [129]
3 years ago
10

What type of reaction is this? N2 + 3H2 2NH3

Chemistry
1 answer:
Levart [38]3 years ago
7 0

Answer:

It is a combination reaction; nitrogen and hydrogen combine to form ammonia.

Explanation:

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14. An enzyme-catalyzed reaction was carried out with the substrate concentration initially a thousand times greater than the Km
emmainna [20.7K]

Answer:

27 min

Explanation:

The kinetics of an enzyme-catalyzed reaction can be determined by the equation of Michaelis-Menten:

v = \frac{vmax[S]}{Km + [S]}

Where v is the velocity in the equilibrium, vmax is the maximum velocity of the reaction (which is directed proportionally of the amount of the enzyme), Km is the equilibrium constant and [S] is the concentration of the substrate.

So, initially, the velocity of the formation of the substrate is 12μmol/9min = 1.33 μmol/min

If Km is a thousand times smaller then [S], then

v = vmax[S]/[S]

v = vmax

vmax = 1.33 μmol/min

For the new experiment, with one-third of the enzyme, the maximum velocity must be one third too, so:

vmax = 1.33/3 = 0.443 μmol/min

Km will still be much smaller then [S], so

v = vmax

v = 0.443 μmol/min

For 12 μmol formed:

0.443 = 12/t

t = 12/0.443

t = 27 min

7 0
3 years ago
Which acid is the acid usually found in your stomach?
amid [387]

Answer:

A.hydrochloric acid

Explanation:

4 0
3 years ago
Calculate the number of kilojoules to warm 125 g of iron from 23.5 °C to 78.0 °C.
insens350 [35]
Given:
Iron, 125 grams T
1 = 23.5 degrees Celsius, T2 = 78 degrees Celsius.  

Required:
Heat produced in kilojoules  

Solution:
The molar mass of iron is 55.8 grams per mole. SO we need to change the given mass of iron into moles.  
 
Number of moles of iron = 125 g/(55.8 g/mol) = 2.24 moles  
<span>
Q (heat) = nRT = nR(T2 = T1)</span>
Q (heat) = 2.24 moles (8.314 Joules per mol degrees Celsius) (78.0 degrees Celsius – 23.5 degrees Celsius)
<u>Q (heat) = 1014.97 Joules or 1.015 kilojoules</u> <span>This is the amount of heat produced in warming 125 g f iron.</span>
7 0
3 years ago
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