Some drain cleaners contain a mixture of sodium hydroxide and aluminum which reacts with water as follows:
2Al(s)+2 NaOH(aq)+6H2O(l)->2Na[Al(OH)4](aq)+3H2(g)
What mass of hydrogen gas can be produced when 5g Al reacts with sufficient NaOH and H2O) according to the above equation?
According to the equation, for each mole of aluminum, one gets 3 moles of H2. So how many moles of Al is 5 grams? You ought to get three times that.
To determine the mass of hydrogen gas produced when 5g of aluminum (Al) reacts with sufficient sodium hydroxide (NaOH) and water (H2O), we can use the stoichiometry of the balanced chemical equation.
The balanced chemical equation is:
2Al(s) + 2NaOH(aq) + 6H2O(l) → 2Na[Al(OH)4](aq) + 3H2(g)
From the balanced equation, we can see that 2 moles of aluminum (Al) react to produce 3 moles of hydrogen gas (H2).
First, we need to calculate the number of moles of aluminum (Al) in 5g using its molar mass. The molar mass of aluminum is 27g/mol.
Number of moles of Al = Mass of Al / Molar mass of Al
Number of moles of Al = 5g / 27g/mol
Next, we determine the number of moles of hydrogen gas (H2) using the mole ratio from the balanced equation.
Number of moles of H2 = Number of moles of Al × (3 moles of H2 / 2 moles of Al)
Finally, we convert the moles of hydrogen gas (H2) to its mass using its molar mass. The molar mass of hydrogen gas is 2g/mol.
Mass of H2 = Number of moles of H2 × Molar mass of H2
By following these steps, you can calculate the mass of hydrogen gas produced when 5g of aluminum reacts with sufficient sodium hydroxide and water according to the provided equation.