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kirill [66]
2 years ago
14

Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid fuel ro

cket motors. The reaction is Fe2O3(s) + 2Al(s) → 2Fe(l) + Al2O3(s) Click here to see the reaction. What is the maximum mass of aluminum oxide that could be produced along with 18.65 g iron?
Chemistry
1 answer:
Diano4ka-milaya [45]2 years ago
3 0

Answer:

16.98 g

Explanation:

The balacend equation is

Fe2O3(s) + 2Al(s) → 2Fe(l) + Al2O3(s)

So, when 2 moles of iron (Fe) are produced, 1 mol of aluminum oxide is produced. The mass molar of the elements are:

Fe = 56 g/mol; O = 16 g/mol; Al = 27 g/mol

Then, the mass molar of Al2O3 is:

2x27 + 3x16 = 102 g/mol

The stoichiometry relation will be:

2 mol of Fe -------------------- 1 mol of Al2O3

2x56 g of Fe -------------------- 102 g of Al2O3

18.65 g of Fe -------------------- x g of Al2O3

By a direct simple three rule:

112x = 1902.3

x = 16.98 g

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Explanation:

4 0
2 years ago
Balance the chemical equation hcl+ Naoh
sattari [20]

Answer:

NaCL + H2O

Explanation:

6 0
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An excess of mg(s) is added to 100.ml of 0.400 m hcl. at 0c and 1 atm pressure, what volume of h 2 (g) can be obtained?
ra1l [238]
The balanced equation for the reaction between Mg and HCl is as follows
Mg + 2HCl --> MgCl₂ + H₂
stoichiometry of HCl to H₂ is 2:1

number of HCl moles reacted - 0.400 mol/L x 0.100 L = 0.04 mol of HCl
since Mg is in excess HCl is the limiting reactant 
number of H₂ moles formed - 0.04/2 = 0.02 mol of H₂

we can use ideal gas law equation to find the volume of H₂
PV = nRT 
where 
P - pressure - 1 atm x 101 325 Pa/atm = 101 325 Pa
V - volume
n - number of moles - 0.02 mol
R - universal gas constant - 8.314 Jmol⁻¹K⁻¹
T - temperature in Kelvin - 0 °C + 273 = 273 K
substituting these values in the equation 

101 325 Pa x V = 0.02 mol x 8.314 Jmol⁻¹K⁻¹ x 273 K
V = 448 x 10⁻⁶ m³
V = 448 mL 
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5 0
3 years ago
What are 2 applications of the Colligative Property that allows freezing point depression?
butalik [34]
1) Adding salt on the roads in the winter time,
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5 0
3 years ago
A compound is 2.00% H by mass, 32.7% S by mass, and 65.3% O by mass. What is its empirical
Katarina [22]

Answer:

empirical formula: H_2SO_4

2 g H

32.7 g S

65.3 g O

Explanation:

Like the problem said, the first thing we can do is calculate the mass of each of the 3 elements in a 100-gram sample:

- 2.00% * 100g = 2 g H

- 32.7% * 100g = 32.7 g S

- 65.3% * 100g = 65.3 g O

Now we need to find the empirical formula from these. To do so, convert all of those masses into moles by using the molar mass for each element:

- the molar mass of H is 1.01 g/mol

- the molar mass of S is 32.06 g/mol

- the molar mass of O is 16 g/mol

2 g H ÷ 1.01 g/mol = 1.98 mol H

32.7 g S ÷ 32.06 g/mol = 1.02 mol S

65.3 g O ÷ 16 g/mol = 4.08 mol O

Our ratio of H : S : O is now:

1.98 mol : 1.02 mol : 4.08 mol

Divide them all by the smallest number, which is 1.02:

1.98/1.02  :  1.02/1.02  :  4.08/1.02

1.94 : 1 : 4

1.94 ≈ 2

So:

2 : 1 : 4

Thus, the empirical formula is: H_2SO_4.

7 0
3 years ago
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