i)
Molar mass of Al = 26.98 g/mol
mass(Al)= 30.0 g
use:
number of mol of Al,
n = mass of Al/molar mass of Al
=(30 g)/(26.98 g/mol)
= 1.112 mol
Since Δ H is negative, heat is released
when 8 mol of Al reacts, heat released = 202.8 kcal
So,
for 1.112 mol of Al, heat released = 1.112*202.8/8 kcal
= 28.19 kcal
Answer: 28.19 kcal
ii)
when -202.8 kcal of heat is involved, 8 mol of Al is reacting
So,
for -1*10^3 kcal, mol of Al = -1*10^3*8/-202.8 kcal
= 39.45 mol
Molar mass of Al = 26.98 g/mol
use:
mass of Al,
m = number of mol * molar mass
= 39.45 mol * 26.98 g/mol
= 1.064*10^3 g
According to balanced equation
mol of Fe2O3 formed = (2/8)* moles of Al
= (2/8)*39.44
= 9.859 mol
Molar mass of Fe2O3,
MM = 2*MM(Fe) + 3*MM(O)
= 2*55.85 + 3*16.0
= 159.7 g/mol
mass of Fe2O3 = number of mol * molar mass
= 9.859*1.597*10^2
= 1.575*10^3 g
Answer:
Mass of Al = 1.064*10^3 g
Mass of Fe2O3 = 1.575*10^3 g
(5) - The following reaction is the thermite reaction used in underwater (and space) welding: 8Als)+Fe,...
(5) - The following reaction is the thermite reaction used in underwater (and space) welding: 8Al+Fe, 036 - A1,03 + 2Fe + 202.8 kcal/mol How many kilocalories of heat are generated when 30.0 g of Al are reacted completely in the above thermite reaction? ii) If you need 1.00x10' kcal of heat, how many grams of Al and Fe2O3 are needed?
(5). The following reaction is the thermite reaction used in underwater (and space) welding: 8A1, +Fe, A1,0 + 2Fe + 202.8 kcal/mol How many kilocalories of heat are generated when 30.0 g of Al are reacted completely in the above thermite reaction? ii) If you need 1.00x10 kcal of heat, how many grams of Al and Fe:Os are needed?
(5) - The following reaction is the thermite reaction used in underwater (and space) welding: 8Al) + Fe, 036) - Al,031 + 2Fe + 202.8 kcal/mol i) How many kilocalories of heat are generated when 30.0 g of Al are reacted completely in the above thermite reaction? ii) If you need 1.00x109 kcal of heat, how many grams of Al and Fe2O, are needed?
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he thermite reaction, used for welding iron, is the reaction of Fe3O4 with Al. 8 Al (s) + 3 Fe3O4 (s) \longrightarrow ⟶ 4 Al2O3 (s) + 9 Fe (s) \Delta Δ H° = -3350. kJ/mol rxn Because this large amount of heat cannot be rapidly dissipated to the surroundings, the reacting mass may reach temperatures near 3000. °C. How much heat (in kJ) is released by the reaction of 16 g of Al with 76.3 g of Fe3O4? Enter...
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