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Mazyrski [523]
2 years ago
13

If predators A and B prey upon the same species and predator A is eliminated, the population of predator B will likely _________

_. a. be eliminated b. increase c. decrease d. remain the same Please select the best answer from the choices provided A B C D
Chemistry
2 answers:
trasher [3.6K]2 years ago
5 0

Answer: B. Increase because there will be more resources for the remaining predators

REY [17]2 years ago
4 0

Answer: B

Explanation: YES

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Which of the following is/are true regarding initial and maximal velocity of enzyme-mediated reactions?
kenny6666 [7]

Answer:

a. True

b. True

c. False

d. True

Explanation:

a). A a very low substrate concentration , $S. Thus according to the Machaelis-Menten equation becomes

$V_0 = \frac{V_{max} \times [S]}{Km}$

Here since the $V_0$ varies directly to the substrate concentration [S], the initial velocity is lower than the maximal velocity. Thus option  (a) is true.

b). The Michaelis -Menten kinetics equation states that :

   $V_0 = \frac{V_{max} \times [S]}{Km+[S]}$

  Here the initial velocity changes directly with the substrate concentration as $V_0$ is directly proportional to [S]. But $V_{max}$ is same for any particular concentration of the enzymes. Thus, option (b) is true.

c). As the substrate concentration increases, the initial velocity also increases. Thus option (c) is false.

d). Option (d) explains the procedures to estimate the initial velocity which is correct. Thus, option (d) is true.

7 0
3 years ago
How many molecules of co2 form when 2.00 g of c2h5oh are produced?
Ronch [10]
The reaction involved in this problem is called the combustion reaction where a hydrocarbon reacts with oxygen to product carbon dioxide and water. The reaction of C2H5OH would be as follows:

C2H5OH + 3O2 = 2CO2 + 3H2O

To determine the number of molecules of CO2 that is formed, we need to determine the number of moles produced from the initial amount of C2H5OH and the relation from the reaction. Then we multiply avogadros number which is equal to 6.022x10^23 molecules per mole. 

2.00 g C2H5OH ( 1 mol C2H5OH / 46.08 g C2H5OH ) ( 2 mol CO2 / 1 mol C2H5OH ) = 0.0868 mol CO2
0.0868 mol CO2 ( 6.022x10^23 molecules / mol ) = 5.23x10^22 molecules CO2
4 0
3 years ago
A 150.0 mL sample of an aqueous solution at 25°C contains 15.2 mg of an unknown nonelectrolyte compound. If the solution has an
inysia [295]

<u>Answer:</u> The molar mass of the unknown compound is 223.2 g/mol

<u>Explanation:</u>

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

\pi=iMRT

where,

\pi = osmotic pressure of the solution = 8.44 torr

i = Van't hoff factor = 1 (for non-electrolytes)

M = molarity of solute = ?

R = Gas constant = 62.3637\text{ L torr }mol^{-1}K^{-1}

T = temperature of the solution = 25^oC=[273+25]=298K

Putting values in above equation, we get:

8.44torr=1\times M\times 62.3637\text{ L. torr }mol^{-1}K^{-1}\times 298K\\\\M=\frac{8.44}{1\times 62.3637\times 298}=4.54\times 10^{-4}M

To calculate the molecular mass of solute, we use the equation used to calculate the molarity of solution:

\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}

We are given:

Molarity of solution = 4.54\times 10^{-4}M

Given mass of unknown compound = 15.2 mg = 0.0152 g   (Conversion factor:  1 g = 1000 mg)

Volume of solution = 150.0 mL

Putting values in above equation, we get:

4.54\times 10^{-4}M=\frac{0.0152\times 1000}{\text{Molar mass of unknown compound}\times 150.0}\\\\\text{Molar mass of unknown compound}=\frac{0.0152\times 1000}{150.0\times 4.54\times 10^{-4}}=223.2g/mol

Hence, the molar mass of the unknown compound is 223.2 g/mol

5 0
3 years ago
I really need help plz I’ll give 40 points
polet [3.4K]
I’m pretty sure it’s b
4 0
3 years ago
Read 2 more answers
Round to 4 significant figures. <br> 0.007062
Monica [59]
.0071 you round 0 to1 because the 6 is bigger than 5 and if anything is bigger than five you round up that last number
7 0
3 years ago
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