a fire extignuisher produces carbon dioxide by the reaction between sodium hydrocarbonate and sulfuric acid. if a fire extinguisher is desgined to hold 600.0g of sodium hydrocarbonate calculate : the mass of sulfuric acid required to react with sodium hydrocarbonate
AND calculate the volume of 12.0 m L^-1 sulfuric acid required to react with the sodium hydrocarbonate
That is sodium hydrogencarbonate, or sodium bicarbonate.
That type of fire extinguisher has not been around many years.
H2SO4+NaHCO3 >> CO2 + H20 + Na2SO4
balance the equation. Then, calculate the moles of sodium bicarbonate you have in 600 grams. From the mole coefficents in the balanced equation, you will know how many moles of H2SO4 you need, and that can be converted to grams.
I will be happy to check your work.
To calculate the mass of sulfuric acid required to react with sodium hydrocarbonate, we need to determine the balanced equation for the reaction first.
The reaction between sodium hydrocarbonate (NaHCO3) and sulfuric acid (H2SO4) can be represented as follows:
2 NaHCO3 + H2SO4 → Na2SO4 + 2 H2O + 2 CO2
According to the balanced equation, for every 2 moles of sodium hydrocarbonate, we need 1 mole of sulfuric acid.
1 mole of sodium hydrocarbonate (NaHCO3) has a molar mass of:
Na = 22.99 g/mol
H = 1.01 g/mol
C = 12.01 g/mol
O = 16.00 g/mol (x3)
Adding these masses together, we get:
22.99 + 1.01 + 12.01 + (16.00 * 3) = 84.01 g/mol
Now, we can calculate the number of moles of sodium hydrocarbonate based on the given mass of 600.0 g:
Moles of sodium hydrocarbonate = mass / molar mass
Moles = 600.0 g / 84.01 g/mol ≈ 7.14 mol
From the balanced equation, we know that 1 mole of sulfuric acid (H2SO4) is needed for every 2 moles of sodium hydrocarbonate.
Therefore, the number of moles of sulfuric acid required is half the number of moles of sodium hydrocarbonate:
Moles of sulfuric acid = 7.14 mol / 2 = 3.57 mol
Finally, to determine the mass of sulfuric acid required, we need to multiply the number of moles by the molar mass of sulfuric acid.
The molar mass of sulfuric acid (H2SO4) is:
H = 1.01 g/mol (x2)
S = 32.07 g/mol
O = 16.00 g/mol (x4)
Adding these masses together, we get:
(1.01 * 2) + 32.07 + (16.00 * 4) = 98.09 g/mol
Mass of sulfuric acid required = moles of sulfuric acid × molar mass of sulfuric acid
Mass = 3.57 mol × 98.09 g/mol ≈ 350.10 g
Therefore, the mass of sulfuric acid required to react with 600.0 g of sodium hydrocarbonate is approximately 350.10 grams.
Now, let's move on to calculating the volume of 12.0 M (molar) sulfuric acid required to react with the sodium hydrocarbonate.
First, we need to convert the given volume of sulfuric acid from milliliters (mL) to liters (L):
Volume in liters = 12.0 mL × (1 L / 1000 mL) = 0.012 L
Next, we can calculate the number of moles of sulfuric acid based on its molarity (M) and volume:
Moles of sulfuric acid = molarity × volume
Moles = 12.0 M × 0.012 L = 0.144 mol
Using the balanced equation, we know that 1 mole of sulfuric acid reacts with 2 moles of sodium hydrocarbonate.
Therefore, the number of moles of sodium hydrocarbonate is twice the number of moles of sulfuric acid:
Moles of sodium hydrocarbonate = 0.144 mol × 2 = 0.288 mol
Thus, the volume of 12.0 M sulfuric acid required to react with the sodium hydrocarbonate is 0.012 L.