Respuesta :
Answer:
1) 1.39 grams H2O2
2) 0.933 grams Fe
Explanation:
Step 1: Data given
Volume of oxygen = 0.460 L
STP = 1 atm and 273 K
Step 2: The balanced equation
2H2O2(aq) → 2H2O(l) + O2(g)
Step 3: Calculate the number of moles O2
p*V = n*R*T
⇒with p= the pressure = 1 atm
⇒with V = the volume = 0.460 L
⇒with n = the number of moles = TO BE DETERMINED
⇒with R = the gas constant = 0.08206 L*atm/mol*K
⇒with T = the temperature = 273 K
n = (p*V)/(R*T)
n = (1 * 0.460)/ (0.08206*273)
n = 0.0205 moles moles
Step 4: Calculate moles H2O2
For 2 moles H2O we'll have 2 moles H2O and 1 mol O2
For 0.0205 moles O2 we'll need 2*0.0205 = 0.041 moles H2O2
Step 5: Calculate mass H2O2
Mass H2O2 = moles H2O2 * molar mass H2O2
Mass H2O2 = 0.041 moles * 34.01 g/mol
Mass H2O2 = 1.39 grams
Step 1: Data given
Volume of hydrogen = 0.500 L
STP = 1 atm and 273 K
Step 2: The balanced equation
3Fe(s) + 4H2O(l) → Fe3O4(s) + 4H2(g)
Step 3: Calculate the moles of H2
p**V = n*R*T
⇒with p= the pressure = 1 atm
⇒with V = the volume = 0.500 L
⇒with n = the number of moles = TO BE DETERMINED
⇒with R = the gas constant = 0.08206 L*atm/mol*K
⇒with T = the temperature = 273 K
n = (p*V) / '*T)
n = (1 * 0.500) / (0.08206 * 273)
n = 0.0223 moles
Step 4: Calculate moles Fe
For 3 moles Fe we need 4 moles H2O to produce 1 mol Fe3O4 and 4 moles H2
For 0.0223 moles H2 we'll need 0.0223 *3/4 = 0.0167 moles Fe
Step 5: Calculate mass of Fe
Mass Fe = moles Fe * atomic mass Fe
Mass Fe = 0.0167 moles * 55.845 g/mol
Mass Fe = 0.933 grams Fe
1. The mass of the hydrogen peroxide should be 1.39 grams H2O2.
2) The mass of the iron should be 0.933 grams Fe.
Calculation of the mass:
Since
Volume of oxygen = 0.460 L
STP = 1 atm and 273 K
Now The balanced equation
2H2O2(aq) → 2H2O(l) + O2(g)
Now the number of moles O2
p*V = n*R*T
Here p= the pressure = 1 atm
V = the volume = 0.460 L
n = the number of moles = ?
R = the gas constant = 0.08206 L*atm/mol*K
T = the temperature = 273 K
Now
n = (p*V)/(R*T)
n = (1 * 0.460)/ (0.08206*273)
n = 0.0205 moles moles
Now moles H2O2 should be
For 2 moles H2O we'll have 2 moles H2O and 1 mol O2
So,
For 0.0205 moles O2 we'll need 2*0.0205 = 0.041 moles H2O2
Now mass H2O2
Mass H2O2 = moles H2O2 * molar mass H2O2
Mass H2O2 = 0.041 moles * 34.01 g/mol
Mass H2O2 = 1.39 grams
2. The mass of the iron should be
Since
Volume of hydrogen = 0.500 L
STP = 1 atm and 273 K
Now
The balanced equation
3Fe(s) + 4H2O(l) → Fe3O4(s) + 4H2(g)
Now the moles of H2
p**V = n*R*T
Here
p= the pressure = 1 atm
V = the volume = 0.500 L
n = the number of moles = ?
R = the gas constant = 0.08206 L*atm/mol*K
T = the temperature = 273 K
So,
n = (p*V) / '*T)
n = (1 * 0.500) / (0.08206 * 273)
n = 0.0223 moles
Now Calculate moles Fe
For 3 moles Fe we need 4 moles H2O to produce 1 mol Fe3O4 and 4 moles H2
So,
For 0.0223 moles H2 we'll need 0.0223 *3/4 = 0.0167 moles Fe
Now the mass of Fe
Mass Fe = moles Fe * atomic mass Fe
Mass Fe = 0.0167 moles * 55.845 g/mol
Mass Fe = 0.933 grams Fe
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