A dilute solution of sulfiric acid is added to 15g of copper and iron mixture.
a) the volume of h2 envolved at standard conditions is 4.48L what is the mass of each of the metals constituting the mixture ?
Vm=24l.mol.
I dont know the answer
i don’t know the answer
To determine the mass of each metal in the mixture, we need to use stoichiometry and the ideal gas law. Here's how you can solve this problem step-by-step:
1. Write a balanced chemical equation for the reaction between sulfuric acid (H2SO4) and copper (Cu) and iron (Fe). The reaction can be represented as follows:
H2SO4 + Cu/Fe → CuSO4/FeSO4 + H2
2. Calculate the number of moles of hydrogen gas (H2) released using the ideal gas law:
PV = nRT
Where:
P = pressure (usually given as standard conditions, which is 1 atm)
V = volume of gas (given as 4.48 L)
n = number of moles
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (usually given as standard conditions, which is 273 K)
Since the volume is given at standard conditions, we can directly use the ideal gas law. Rearranging the equation, we have:
n = PV/RT
= (1 atm) * (4.48 L) / (0.0821 L·atm/mol·K * 273 K)
Calculate the value of n.
3. Determine the mole-to-mole ratio between the reactant (H2SO4) and the product (H2) using the balanced equation from step 1. Since we don't know the specific reactant (copper or iron), we need to consider both possibilities separately.
For copper:
1 mole of H2SO4 reacts with 1 mole of Cu
Therefore, n_Cu = n_H2SO4
For iron:
1 mole of H2SO4 reacts with 1 mole of Fe
Therefore, n_Fe = n_H2SO4
4. Calculate the molar mass of copper (Cu) and iron (Fe) using the atomic masses from the periodic table.
5. Calculate the mass of each metal using the moles determined in step 2 and the molar masses determined in step 4.
mass_Cu = n_Cu * molar mass_Cu
mass_Fe = n_Fe * molar mass_Fe
By following these steps, you should be able to determine the mass of each metal (copper and iron) in the mixture.