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3 years ago

Is the cell membrane a factory part or worker? Please explain what it does as a factory part or worker

Chemistry

2 answers:

lozanna [386]3 years ago

7 0

Answer:

hey i saw you asked about the kinetic energy lab report on edg and i was wondering if you ever finished it and could send it me plzzzzzzzz

Explanation:

Tema [17]3 years ago

3 0

It is probably a worker bc it lets things in and out of the cell and stops harmful things from entering the cell

You might be interested in

What volume of a 0.550 M solution of potassium hydroxide (KOH) can be made with 19.9 g of potassium hydroxide?

Natalija [7]

Answer:

0.645 L

Explanation:

To find the volume, you need to (1) convert grams to moles (using the molar mass) and then (2) calculate the volume (using the molarity ratio). The final answer should have 3 sig figs to match the sig figs of the given values.

(Step 1)

Molar Mass (KOH): 39.098 g/mol + 15.998 g/mol + 1.008 g/mol

Molar Mass (KOH): 56.104 g/mol

19.9 grams KOH 1 mole
-------------------------- x ----------------------- = 0.355 moles KOH
56.014 grams

(Step 2)

Molarity = moles / volume <----- Molarity ratio

0.550 M = 0.355 moles / volume <----- Insert values

(0.550 M) x volume = 0.355 moles <----- Multiply both sides by volume

volume = 0.645 L <----- Divide both sides by 0.550

6 0

1 year ago

A scientist prepared an aqueous solution of a 0.45 M weak acid. The pH of the solution was 2.72. What is the percentage ionizati

aleksandr82 [10.1K]

Answer:

0.42%

Explanation:

∵ pH = - log[H⁺].

2.72 = - log[H⁺]

∴ [H⁺] = 1.905 x 10⁻³.

∵ [H⁺] = √Ka.C

∴ [H⁺]² = Ka.C

∴ ka = [H⁺]²/C = (1.905 x 10⁻³)²/(0.45) = 8.068 x 10⁻⁶.

∵ Ka = α²C.

Where, α is the degree of dissociation.

∴ α = √(Ka/C) = √(8.065 x 10⁻⁶/0.45) = 4.234 x 10⁻³.

∴ percentage ionization of the acid = α x 100 = (4.233 x 10⁻³)(100) = 0.4233% ≅ 0.42%.

4 0

3 years ago

Read 2 more answers

How many grams of MgO are needed to produce 264.0 grams of Mg(OH)2?

sergij07 [2.7K]

15396 g
tell me if its correct

7 0

3 years ago

Please help!! I have 10 minutes left!!

Licemer1 [7]

Explanation:

1 is a process that occurs when gases in earth's atmosphere trap the sun's heat .

2 . heat in the atmosphere to warm the planet .

I only know the first too sorry ✨

8 0

3 years ago

One of the reactions that occurs in a blast furnace, in which iron ore is converted to cast iron, is Fe2O3 + 3CO → 2Fe + 3CO2 Su

Tpy6a [65]

Answer : The percent purity of $Fe_2O_3$ in the original sample is 87.94 %

Explanation :

The given balanced chemical reaction is:

$Fe_2O3+3CO\rightarrow 2Fe+3CO_2$

First we have to calculate the mass of Fe.

$\text{Moles of }Fe=\frac{\text{Mass of }Fe}{\text{Molar mass of }Fe}$

Molar mass of Fe = 55.8 g/mole

$\text{Moles of }Fe=\frac{1.79\times 10^3kg}{55.8g/mole}=\frac{1.79\times 10^3\times 1000g}{55.8g/mole}=3.15\times 10^4mole$

Now we have to calculate the moles of $Fe_2O_3$

From the balanced chemical reaction we conclude that,

As, 2 moles of Fe produced from 1 mole of $Fe_2O_3$

So, $3.15\times 10^4mole$ of Fe produced from $\frac{3.15\times 10^4}{2}=15750$ mole of $Fe_2O_3$

Now we have to calculate the mass of $Fe_2O_3$

$\text{ Mass of }Fe_2O_3=\text{ Moles of }Fe_2O_3\times \text{ Molar mass of }Fe_2O_3$

Molar mass of $Fe_2O_3$ = 159.69 g/mole

$\text{ Mass of }Fe_2O_3=(15750moles)\times (159.69g/mole)=2.515\times 10^6g=2.515\times 10^3kg$

Now we have to calculate the percent purity of $Fe_2O_3$ in the original sample.

Mass of original sample = $2.86\times 10^3kg$

$\text{Percent purity}=\frac{\text{Mass of }Fe_2O_3}{\text{Mass of sample}}\times 100$

$\text{Percent purity}=\frac{2.515\times 10^3kg}{2.86\times 10^3kg}\times 100=87.94\%$

Therefore, the percent purity of $Fe_2O_3$ in the original sample is 87.94 %

3 0

2 years ago