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can 4 Al(s) +30₂ (9) -> 2Al2O₃ (3) A what mass of Al 82.49 AL oxice...
3. Determine the limiting reactant and the mass of AlCl3 produced by reacting 15.0 g of Al with 30.0 g of Cly according to the following chemical equation. The molar mass of AICI is 133.33 g/mol. A1 = 26.98 g/mol 2 Al(s) + 3 Cl2 (g) → 2 AlCl3(s) C1 = 35.45 g/mol A) Al is the limiting reactant, 32.4 g of AlCl3 produced. B) Al is the limiting reactant, 74.1 g of AlCl3 produced. C) Cl2 is the limiting...
1. Aluminum reacts with oxygen according to the following reaction: 4 Al(s) + 3 O2(g) -> 2 Al2O3 If 8.00 moles of oxygen are reacted with 8.00 moles of aluminum to completion, which is the excess reactant?
Aluminum oxide (Al2O3) is produced according to the following equation. 4 Al(s) + 3 O2(g) → 2 Al2O3(s) If the reaction occurs with an 82.4% yield, what mass of aluminum should be reacted with excess oxygen to produce 45.0 grams of Al2O3? a. 54.6 g Al b. 37.9 g Al c. 35.1 g Al d. 23.8 g Al e. 28.9 g Al How do we solve this problem
Calculate Moles of oxygen needed to react with 4.21 mol of Al. What mass of Al2O3 should be produced? 4 Al (s) + 3 O2 (g) → 2 Al2O3 (s)
Consider the reaction between HCl and 02: 4 HCl + O2 ---------------> 2 H2O + 2 Cl2 Calculate the theoretical vield of H O when 64 grams of HCl react with 19 grams of 02. O A. 16 g H20 O B.21 g H20 C.32 g H20 O 0.43 g H20 10 points TANO 4 Al + 302 ---------------> 2 Al2O3 If 12.85 g of Al reacts completely with oxygen and 18.42 g of aluminum oxide is obtained, what is...
The 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) 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 19.3 g of Al with 63.2 g of Fe3O4? Enter a...
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...
The student synthesise aluminum oxide according to this reaction: 4 Al(s) + 3 0,(9) + 2 A1,0,(s) Considering the mass of the limiting reactant she used, the student worked out that the theoretical yield of Al,0, is 3.208 g. She obtained an experimental yield of 2.329 g. What is the percentage yield for her synthesis? Answer:
4. Consider the reaction of aluminum and oxygen: Al(s) + O2(g) Al2O3(s) (i). Which is the limiting reactant if we start with 30.0 g Al and 30.0 g O2? (ii). What is the Theoretical Yield for the reaction? (iii). If 25.85 g of Al2O3 was collected at the completion of the reaction (actual yield), what is the % yield for the reaction? 5. (a). A 1.506-g sample of limestone-containing material gave 0.558 g of...
3.(15pts) In each case, find the missing AH. (kJ/mole) (a) If 2 Al(s) + Fe2O3(s) ----> Al2O3(s) + 2 Fe(s) AH,xº = -851.5kJ/mol then 1/8 Al2O3(s) + 1/4 Fe(s) --> 1/4 Al(s) + 1/8 Fe2O3(s) AHX = ? (b) If CaO(8) + 3 C(s) --> CaC2(s) + CO(g) AH,” = 464,8 kJ/mol then 6 CaO(s) + 18 C(s) ---> 6 CaCz(s) +6 CO(g) AHX = ? (c) If N2(g) + 2 O2(g) ---> N204(g) and 2 NO2(g) ----> N2(g) +...