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Lana71 [14]
3 years ago
13

Describe how you could use two LB/agar plates, some E. coli, and some ampicillin to determine how E. coli cells are affected by

ampicillin.
Chemistry
1 answer:
KiRa [710]3 years ago
8 0

Answer:

For this experiment we are going to take plate 1 as the control plate, so, in it there will be just E. coli in LB/agar; in plate 2, we are going to put E. coli in LB/agar and some ampicillin.  Then, we have to wait for the E. coli colonies to form. After a while, the E. coli growth can be compared on both plates and determine if ampicillin affects or not the E. coli colonies.

Explanation:

If the ampicillin affects negatively E. coli colonies, we are going to observe that in plate 1 (control plate) there are E. coli colonies growing, but in plate 2, there is no E. coli colonies or, at least, there is a fewer number of colonies on it. If ampicillin doesn't affect E.coli, plate 1 (control) and plate 2 (ampicillin experiment) are going to be similar in number of colonies.

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Assuming the metals lose all their valence electrons and the nonmetals gain electrons to complete the s-p subshells, which listi
Nataly [62]

Answer: Option (c) is the correct answer.

Explanation:

Atomic number of sodium is 11 and its electronic configuration is 1s^{2}2s^{2}2p^{6}3s^{1}. When sodium loses one electron then it will attain +1 charge and its electronic configuration will be as follows.

Na^{+} : 1s^{2}2s^{2}2p^{6}

Atomic number of fluorine is 9 and its electronic configuration is 1s^{2}2s^{2}2p^{5}. When fluorine gains an electron then it acquires -1 charge and its electronic configuration is as follows.

F^{-} : 1s^{2}2s^{2}2p^{6}

Atomic number of aluminium is 13 and its electronic configuration is 1s^{2}2s^{2}2p^{6}3s^{2}3p^{1}. When aluminium loses its valence electrons then it acquires +3 charge and its electronic configuration is as follows.

Al^{3+} : 1s^{2}2s^{2}2p^{6}

Thus, we can conclude that the listing for aluminum is correct.

8 0
3 years ago
Most of the sulfur used in the United States is chemically synthesized from hydrogen sulfide gas recovered from natural gas well
Rom4ik [11]

Answer:

The rate at which sulfur dioxide is being produced is 0.90 kg/s.

Explanation:

Volume of oxygen gas consumed in second ,V= 994 L

Pressure of the gas = p

Temperature of the gas = T = 170°C= 170 + 273 K=443 K

Moles of oxygen gas consumed in a second = n

PV=nRT ( ideapl gas equation)

n=\frac{PV}{RT}=\frac{0.77 atm\times 994 L}{0.0821 atm L/mol K\times 443 K}

n = 21.044 mole

Moles of dioxygen gas consumed per second = 21.044 mol

2H_2S(g)+3O_2(g)\rightarrow 2SO_2(g)+2H_2O(g)   (Claus process)

According to reaction, 3 moles of dioxygen gives 2 moles of sulfur dioxide gas.Then 21.044 moles of dioxygen will give;

\frac{2}{3}\times 21.044 ol=14.029 mol of sulfur dioxide

Mass of 14.029 moles of sulfur dioxide gas;

14.029 mol × 64 g/mol = 897.86 g

897.86 g = 0.89786 kg ≈ 0.90 kg

Mass of sulfur dioxide produced per second = 0.90 kg

The rate at which sulfur dioxide is being produced is 0.90 kg/s.

7 0
4 years ago
11. Fill in the blanks below for a general chemical reaction (products, reactants).
Bad White [126]
Reactants on the left and products on the right
5 0
3 years ago
Which of the following is a chemical property of seawater
Kaylis [27]

Answer:

A ( salinity )

Explanation:

The full question is actually:

Which of the following is a chemical property of seawater?

salinity

temperature

density

depth

Hope it helps

Put a thanks

Thank you

3 0
3 years ago
2KCIO3 ----------&gt; 2KCI + 302<br> How many moles of KCIO3 are needed to make 3.5 moles of KCL?
lyudmila [28]

Answer:

3.5 mol KClO3

Explanation:

Given 3.50 moles of KCl as the target amount in the problem, used the coefficient of the balanced chemical reaction involved to determine the number of moles of potassium perchlorate needed.

x mole of  KClO3  = 3.5 mol  KCl x [(2 mol KCl)/ (2 mol KClO3)] = 3.5 mol KClO3

x mole of  KClO3 = 3.5 mol KClO3

3 0
3 years ago
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