A S.T.P.how many litres of hydrogen can be obtained from the reaction of 500cm3 of 0.5M H2SO4 with excess zinc metals?(molar volume of H2 at stp=22.4dm3).
you are told that 1 mole of gas fills 22.4 Liters
so, how many moles of H2 were produced?
To determine the number of liters of hydrogen gas (H2) that can be obtained from the reaction of 500 cm3 of 0.5 M H2SO4 with excess zinc (Zn) metal, we need to follow these steps:
Step 1: Write the balanced chemical equation for the reaction:
Zn + H2SO4 -> ZnSO4 + H2
Step 2: Determine the number of moles of H2SO4:
Volume of H2SO4 = 500 cm3 = 500/1000 = 0.5 L
Molarity of H2SO4 = 0.5 M
Moles of H2SO4 = Molarity x Volume
Moles of H2SO4 = 0.5 M x 0.5 L = 0.25 moles
Step 3: Use the stoichiometry of the balanced equation to find the number of moles of H2:
From the balanced equation, we see that 1 mole of H2SO4 produces 1 mole of H2.
Therefore, moles of H2 = 0.25 moles
Step 4: Convert moles of H2 to liters of H2 at STP:
1 mole of any gas occupies 22.4 L at STP.
Therefore, volume of H2 at STP = 0.25 moles x 22.4 L/mole = 5.6 L
So, the reaction of 500 cm3 of 0.5 M H2SO4 with excess zinc metal will produce 5.6 liters of hydrogen gas at STP.
To determine how many liters of hydrogen can be obtained from the given reaction, we need to use stoichiometry. The balanced chemical equation for the reaction between sulfuric acid (H2SO4) and zinc (Zn) is:
Zn + H2SO4 -> ZnSO4 + H2
From the equation, we see that for every 1 mole of zinc reacted, 1 mole of hydrogen is produced. Additionally, we need to consider the molar volume of hydrogen gas at STP (Standard Temperature and Pressure), which is 22.4 dm^3/mol.
Let's proceed with the calculations:
Step 1: Calculate the number of moles of H2SO4 using the given volume and concentration:
Molarity (M) = Moles (mol) / Volume (L)
Given volume = 500 cm^3 = 0.5 L
Given concentration = 0.5 M
Moles of H2SO4 = Concentration x Volume = 0.5 M x 0.5 L = 0.25 mol
Step 2: Since there is excess zinc, all the moles of H2SO4 will react with the same number of moles of Zn to produce H2.
Therefore, the number of moles of hydrogen (H2) produced is also 0.25 mol.
Step 3: Finally, use the molar volume at STP to convert the number of moles of hydrogen into liters.
Volume (L) = Moles (mol) x Molar volume (L/mol)
Volume of H2 = 0.25 mol x 22.4 dm^3/mol = 5.6 dm^3
So, from the reaction of 500 cm^3 of 0.5 M H2SO4 with excess zinc, we can obtain 5.6 liters of hydrogen gas at STP.