Convert 50g of calcium carbonate, CaCO3, into moles
convert 50g of calcium carbonate, CaCO3, into moles - 1


Answer 1
Answer: Answer:
            Moles  =  0.5 mol


Moles is related to mass as follow,

                                       Moles  =  Mass / M.mass   ----- (1)

           Mass  =  50 g

           M.mass  =  Ca (40) + C (12) + O₃ (16)₃  =  100 g/mol

Putting values in equation 1,

                                        Moles  =  50 g ÷ 100 g.mol⁻¹

                                        Moles  =  0.5 mol

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According to the equation below, which of the following will cause the concentration of H2SO4 to increase? 2NaHCO3 (s) + H2SO4 (aq) ⇄ Na2SO4 (aq) + 2H2O (l) + 2CO2 (g) View Available Hint(s) According to the equation below, which of the following will cause the concentration of H2SO4 to increase? 2NaHCO3 (s) + H2SO4 (aq) ⇄ Na2SO4 (aq) + 2H2O (l) + 2CO2 (g) addition of some NaHCO3 (s) addition of some Na2SO4 (aq) removal of some H2O (l) removal of some CO2 (g)



Addition of some Na₂SO₄ (aq).


2NaHCO₃ (s) + H₂SO₄ (aq) ⇄ Na₂SO₄ (aq) + 2H₂O (l) + 2CO₂ (g)

According to the Le Chatelier's principle, the addition of Na₂SO₄ to the reaction would lead to shift to the direction of the reaction that consumes Na₂SO₄, in order to reestablish equilibrium. Since the reaction that consumes Na₂SO₄ is the reaction that produces H₂SO₄, the concentration of H₂SO₄ would increase.

What is the atomic number of an element containing 12 neutrons and having a mass number of 24


The element is magnesium, its atomic number is 12.

Calculate the molality of a 35.4 % (by mass) aqueous solution of phosphoric acid (H3PO4) (35.4 % means 35.4 g of H3PO4in 100 g of solution)



3.6124 m/kg


Molality is calculated as moles of solute (mol) divided by kilogram of solvent (kg). Here, we can find these numbers by using the 35.4%, which gives us  35.4 g of H3PO4 and 100 g of solution to work with.

To go from grams to moles for the phosphoric acid, you need to find the molar mass of the compound or element and divide the grams of the compound or element by that molar mass.

Here, the molar mass for phosphoric acid is 97.9952 g/mol. The equation would look like this:

35.4 g x 1 mol / 97.9952 g = 0.3612422 mol

Next, the 100 g of solvent can easily be converted to 0.1 kg of solvent.

To find the molality, divide the moles of solute and kilograms of solution.

0.3612422 mol / 0.1 kg = 3.6124 m/kg

A biochemist studying breakdown of the insecticide DDT finds that it decomposes by a first-order reaction with a half-life of 12.0 yr. How long does it take DDT in a soil sample to decompose from 809 ppbm to 10.0 ppbm (parts per billion by mass)



76.0 years


Step 1: Given data

  • Half-life (t1/2): 12.0 y
  • Initial concentration of DDT ([A]₀): 809 ppbm
  • Final concentration of DDT ([A]): 10.0 ppbm
  • Time elapsed (t): ?

Step 2: Calculate the rate constant (k)

We will use the following expression.

k = ln 2/ t1/2 = ln 2 / 12.0 y = 0.0578 y⁻¹

Step 3: Calculate the time elapsed

For a first-reaction order, we will use the following equation.

ln [A]/[A]₀ = -k × t

t = ln [A]/[A]₀ / (-k)

t = (ln 10.0 ppbm/809 ppbm) / (-0.0578 y⁻¹)

t = 76.0 y

When the reaction mixture is worked-up, it is first washed three times with 5% sodium bicarbonate, and then with a saturated nacl solution. explain why?



After the reaction of mixture is worked-up Washing three times the organic  with sodium carbonate helps to decrease the solubility of the organic layer into the aqueous layer. This allows the organic layer to be separated more easily.

And then the reaction washed by saturated NACL we have The bulk of the water can often be removed by shaking or "washing" the organic layer with saturated aqueous sodium chloride (otherwise known as brine). The salt water works to pull the water from the organic layer to the water layer.

What is the isoelectric point of proteins?


Isoelectric point. The isoelectric point (pI, pH(I), IEP), is the pH at which a particular molecule carries no net electrical charge in the statistical mean. The standard nomenclature to represent the isoelectric point is pH(I), although pI is also commonly seen, and is used in this article for brevity.
The isoelectric point (pI, pH(I),IEP), is the pH at which a particular molecule carries no net electrical charge in the statistical mean.