Answer:
Explanation:
The reaction for the above condition is
Fe(ClO4)3 (s) -> FeCl3 (s) + 6 O2 (g)
We have to calculate the number of moles of Fe(ClO4)3
First step
calculate the number of moles of Fe(ClO4)3
Given
Molar mass of Fe(ClO4)3 = 354.20g/mol
Given mass = 1.52 g
Number of moles of Fe(ClO4)3 = ?
Number of moles of Fe(ClO4)3 = Given mass / Molar mass
= 1.52/ 354.20 = 0.00429 moles of of Fe(ClO4)3
Second step
Calculation of number of moles of oxygen
As we know that from the reaction
1 mole of Fe(ClO4)3 gives = 6 moles of oxygen
0.00429 moles of Fe(ClO4)3gives = 0.00429 x 6
=0.0257 moles of oxygen
Third step Calculation of volume At STP
according to ideal gas law
given Pressure = 1 atm Temperature = 273 k
n number of moles= 0.0257 moles
R ideal gas constant= R = 0.0821 Latmmol-1K-1
Volume = ?
Ideal gas law= PV=nRT
So solving for V= nRT/P
= 0.0257x0.0821x273/ 1
= 0.576 liter= 576 ml
576 ml volume of oxygen gas should be produced under conditions of STP from a 1.52-g sample of Fe(ClO4)3.
