The reaction of Aluminum with oxygen can be written as follows:
To balance the number of O atoms on both side, we cross multiply the number of oxygens. i.e. we multiply 2 on Al2O3 and multiply 3 on O2.
Next, to balance the number of Al atom, we realise that there are 4 Al on right and only one on left. Hence, we multiply 4 on Al to get the balanced reaction.
Now, mass of Aluminum allowed to react with oxygen is 62.79 g.
Atomic mass of Al = 26.98 g/mol
Hence, number of moles of Aluminum in 62.79 g can be calculated as
Hence, there are 2.327 mol of Al in the given amount of Aluminum.
Note that from the balanced equation, 4 mol of Aluminum forms 2 moles of Aluminum oxide.
Hence, the given 2.327 mol of Aluminum above will be able to form:
Hence, 1.164 mol of Al2O3 approximately can be formed from the given amount of Al.
Molar mass of Al2O3 = 101.96 g/mol
Hence, mass of Al2O3 in 1.1635 mol of Al2O3 can be calculated as
Hence, approximately 118.6 g of Al2O3 can be formed from the given amount of Al.
help me do the correct math 25. (12 pts) Aluminum oxide forms when aluminum-reacts with oxygen. Balance the followi...
1. When 15.4 g of aluminum (26.98 g/mol) reacts with 14.8 g of oxygen gas (32.00 g/mol), what is the maximum mass (in grams) of aluminum oxide (101.96 g/mol) that can be produced? 4 Al(s) + 3 O2(g) → 2 Al2O3(s) 2. If 14.1 moles of Cu and 48.7 moles of HNO3 are allowed to react, how many moles of excess reactant will remain if the reaction goes to completion? Cu + 8 HNO3 → 3Cu(NO3)2 + 2NO + 4H2O...
Marked out of 1.00 Aluminum reacts with oxygen to form aluminum oxide according to the following unbalanced equation: Al(s) + O2 (g) → Al2O3 (s) If 5.0 moles of A react with excess oxygen, how many moles of Al2O3 can be produced? Select one: a. 1.0 mole b. 2.0 mole c. 3.0 mole d. 2.5 mole e. 10.0 mole Clear my choice Question 11 Not yet answered
X 1. Aluminum reacts with oxygen to produce aluminum oxide 4 Al(s) + 3 O2(g) + 2 Al2O3(s) IF 3.0 moles of Alreact with excess O2, how many moles of AlzO3 can be formed? a) 1.0 mol b) 1.50 mol c) 3.0 mol d ) 4.0 mol e) 4.5 mol 10. What is the log of 5,400.05? a) 3.07 b) 3.37 c) 3.73 d) 37.32 e) 37.23 Short Answer Questions (True or False)
Could someone help solve? I think i'm not balancing the sides correctly When aluminum oxide reacts with sulfuric acid, aluminum sulfate and water are produced. The balanced equation for this reaction is: AL2O3(s) + 3H2SO4(AQ) ----> AL2(SO4)3(AQ) + 3H2O(L) If 4 moles of aluminum oxide react, The reaction consumes _______moles of sulfuric acid. The reaction produces _______moles of aluminum sulfate and moles of water
DATE 1. How many moles of Na are there in 47.3 g of Na? 2. Calculate the number of grams of sulfur in 112.4 moles of sulfur. 3. Calculate number of atoms in 4.6 g of calcium. 4. How many H atoms are in 272.5 g of methanol, CH0? 5. For the given reaction N, (g) +3H,(g)->2NH(g) a. How many moles of NH, are formed by the complete reaction of 0.154 moles of H? b. How many grams of NH,...
Aluminum hydroxide reacts with sulfuric acid as follows: 2Al(OH)3(s)+3H2SO4(aq)→Al2(SO4)3(aq)+6H2O(l) a. Which reagent is the limiting reactant when 0.450 mol Al(OH)3 and 0.450 mol H2SO4 are allowed to react? b. How many moles of Al2(SO4)3 can form under these conditions? c. How many moles of the excess reactant remain after the completion of the reaction?
1. (12 pts) For the balanced equation below, determine how many grams of UF4 (MW: 314.0 g/mol) can be produced when 7.31 kg of UO2 (MW: 270.0 g/mol) react with 3.94 L of 3.54 M HF (MW: 20.01 g/mol). UO2(g) + 4 HF(aq) → UF4(g) + 2 H20(1) 2. (12 pts) A) Determine how much chromium metal can be produced when 284.54 g of chromium (III) oxide reacts with excess aluminum according to the reaction below. Cr2O3(s) + 2 Al(n)...
conversion factors needed: molar masses of O, and Ho, and molar ratio between Ozand Ho. Molar mass Oz: 2 x 16.00 g/mol = 32.00 g/mol Molar mass HO: (2x 1,01 g/mol)*16.00 /mol 7HO-1.5 80xmor 2 mol No1802 1,0 52.00 gomolo 1 .689 = 1.7 HO Now let's try some problems Be sure to give your answers with the correct number of significant figures. 1. Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs,...
26. Aluminum oxide, Al:O, is used as a filler for paints and varnishes as well as in the manufacture of electrical insulators. Caleulate the mumber of moles in 47.51 g of Al:O A) 2.377 mol B) 2.146 mol C) 1.105 mol ) 0.4660 mol E) 0.4207 mol 27. Calculate the molar mass of rubidium carbonate, Rb COs. A) 340.43 g/mol B) 255.00 g/mol &) 230.94 g/mol D) 145.47 g/mol E) 113.48 g/mol 28. Calculate the molar mass of tetraphosphorus decaoxide,...
E: How many moles of aluminum ions are present in 0.32 moles of Al2(SO4)3? F: How many moles of sulfate ions (SO42?) are present in 1.3 moles of Al2(SO4)3? G: Calculate molar mass C6H14O6 (sorbitol) Express your answer to two decimal places and include the appropriate units. H: The sedative Demerol hydrochloride has the formula C15H22ClNO2. How many grams are in 0.025 moles of Demerol hydrochloride? I: How many moles of H2 are needed to react with 0.55 mol of...