How many grams of soda ash would be needed to produce 1.00 kg of sodium bicarbonate?

736.1 g of soda ash

Explanation:

Data given:

Amount of sodium bicarbonate = 1 Kg

convert Kg to g

1 Kg = 1000 g

Amount of soda ash needed = ?

Solution:

First we look for the reaction by which soda ash gives sodium bicarbonate.

Chemical formulas

c NaHCO₃

Soda Ash = Na₂CO₃

So the reaction is given below:

                    Na₂CO₃ + H₂O + CO₂ > 2 NaHCO₃

So,

now look for the amount of soda ash and NaHCO₃

                   Na₂CO₃ + H₂O + CO₂ > 2 NaHCO₃

                     1 mole                                           2 mole

As,

one mole of Na₂CO₃ (soda ash) gives 2 moles of sodium bicarbonate (NaHCO₃).

Now convert moles to mass

For which molar masses are given below

Molar mass of Na₂CO₃ = 106 g/mol

Molar mass of NaHCO₃ = 72 g/mol

So,

         Na₂CO₃      +       H₂O     +     CO₂      >    2 NaHCO₃

   1 mole (106 g/mol)                                                    2 mole (72 g/mol)

          106 g                                                                            144 g

Apply unity formula

            106 g of Na₂CO₃ ≅ 144 grams NaHCO₃

                X g of Na₂CO₃ ≅ 1000 grams NaHCO₃

Do cross multiplication

              X g of Na₂CO₃ = 106 g x 1000 g / 144 g

               X g of Na₂CO₃ = 736.1 g

So, 736.1 g of soda ash needed to produce 1000 g or 1 kg of sodium bicarbonate.

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

it should be all of them because it asks if you included all of those in your answer

explanation: