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IrinaVladis [17]
3 years ago
5

I need help. It’s due tonight. Thanks

Chemistry
2 answers:
VikaD [51]3 years ago
4 0

Answer:

(a) Streptococcus - Pro

(b) Yeast - Euk

(c) A euglena - Pro

(d) Acidophilus -Pro

shepuryov [24]3 years ago
4 0
All of them are prokaryotes except for yeast because it’s cells have membrane bound nuclei
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Converts 800kg into ng
elixir [45]

Answer:

yes

Explanation:

5 0
3 years ago
student plans to isolate chlorophyll, mix it in a solution of carbon dioxide and water, and then shine light on the mixture. Do
Inga [223]

Answer:

No

Explanation:

<u>In order for glucose to be produced inside the mixture, photosynthesis has to take place</u>. The photosynthetic process requires a series of steps within an organelle called the <u>chloroplast</u>. The chloroplast contains the chlorophyll and other enzymes that are necessary for photosynthesis.

<em>Once the chlorophyll is isolated, it becomes separated from the enzymes necessary for the completion of photosynthesis, and the process is truncated. </em>When light is shined on the mixture, the majority would instead be lost as heat while some cause the chlorophyll molecules to glow.

7 0
3 years ago
(6 points) Calculate the maximum number of moles and grams of H2S that can form when 158 g of aluminum sulfide reacts with 131 g
Schach [20]

Answer:107.1 g, 124.1 g

Explanation:

The equation of the reaction is;

Al2S3(s) + 6H20(l) ----> 2Al(OH)3(s) + 3H2S(g)

Hence;

For Al2S3

Number of moles= reacting mass/molar mass

Number of moles = 158g/150gmol-1 =1.05 moles

If 1 mole of Al2S3 yields 3 moles of H2S

1.05 moles of Al2S will yield

1.05 × 3/1 = 3.15 moles

Mass of H2S = 3.15moles × 34 gmol-1 = 107.1 g

For water

Number of moles of water = 131g/18gmol-1= 7.3 moles

6 moles of water yields 3 moles of H2S

7.3 moles of water will yield 7.3 × 3/6 = 3.65 moles of H2S

3.65 moles × 34 gmol-1 =124.1 g

5 0
3 years ago
How many moles of Ca(OH)2 are in 3.5kg of Ca(OH)2? Answer in units of mole
Kobotan [32]
First, you need to convert kg to g. 
So, 1 kg =1000g.
3.5 x 1000 = 3500g Ca(OH)2

We need to know the molar mass of Ca(OH)2. 
Ca= 40.08 g
O=2(15.999)
H=2(1.0079)

Add them all together and you get 74.0938 g.

Put it in the formula from mass to moles. 

# of moles = grams Ca(OH)2 x 1 mol Ca(OH)2
                                                  --------------------
                                                  molar mass Ca(OH)2

3500 g Ca(OH)2 x 1 mol Ca(OH)2
                              ---------------------
                             74.0938 g Ca(OH)2

So divide 1/74.0938 and multiply by 3500.

You will get about 47.24 moles Ca(OH)2.

Hope this helps! :)
7 0
3 years ago
Read 2 more answers
How much heat is lost when 575 grams molten iron at 1825 k becomes solid iron at 293 k? The melting point or iron is 1811 k.​
Galina-37 [17]

Answer:

146 kJ  

Explanation:

There are two heat flows in this question.  

Heat lost on cooling + heat lost on solidifying = 0  

                 q₁              +                 q₂                   = 0  

              mCΔT          +             nΔHsol              = 0  

Data:  

       m = 575 g  

       C = 0.449 J·K⁻¹g⁻¹  

    T_i = 1825 K  

    T_f = 1811 K  

ΔHsol = -13.8 kJ·mol⁻¹  

Calculations:  

(a) Heat lost on cooling  

ΔT = T_f - T_i = 1811 K - 1825 K = -14 K  

q₁ = mCΔT = 575 g × 0.449 J·K⁻¹g⁻¹ × (-14 K) = -361 J = -3.61 kJ  

(b) Heat lost on solidifying  

n = \text{575 g} \times \dfrac{\text{1 mol}}{\text{55.84 g}} = \text{10.30 mol}\\\\q_{2} = n\Delta_{\text{sol}}H = \text{10.30 mol} \times \dfrac{\text{-13.8 kJ}}{\text{1 mol}}= \text{-142.1 kJ}

(c) Total heat lost  

q = q₁ + q₂ = -3.61 kJ - 142.1 kJ = -146 kJ  

The heat lost was 146 kJ.

 

5 0
3 years ago
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