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Determine all possible ratios for the following balanced chemical equations. a) 4Al(s) + 3O2(g)→2Al2O3(s) b) 3Fe(s) + 4H2O(l) → Fe3O4(s) + 4H2(g)
a) Al:O= 4:3Al: Al2O3= 2:1O: Al2O3= 3:2b)Fe: H2O= 3:4Fe:Fe3O4= 3:1Fe: H2 = 3: 4
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Aluminum oxide is decomposed using electricity to produce aluminum metal. Hm grams of aluminum metal can be produced from 100.0g of Al2O3?
2Al2O3--> 4Al+ 3O2
If 2Al2O3 --gt; 4Al+ 3O2; So, first of all we can find amount of substance of Al2O3: n(Al2O3) = m(Al2O3)/M(Al2O3); M(Al2O3) = Ar(Al)*2 + Ar(O) *3; M(Al2O3) = 27*2+16*3 =...
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When heated, KClO3 decomposes into KCl and O2.
2KClO3= 2KCl + 3O2
If this reaction produced 17.2 g of KCl, how many grams of O2 were produced?
According to the reaction, number of moles of KCl and O2 produced during the decomposition must be equal. As a result, the mass of oxygen equals:m(O2) = [m(KCl) × 3...
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According to the following equation, how many moles of aluminum are needed to form 3.7 mol Al2O3?
4Al + O2
Solution:The balanced chemical equation:4Al + 3O2 = 2Al2O3According to the chemical equation: n(Al)/4 = n(Al2O3)/2n(Al)/2 = n(Al2O3)n(Al) = 2 × n(Al2O3)Hence,n(Al) = 2 × 3.7 mol = 7.4 molMoles of...
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how many moles of iron (III) is produced by 0.030 moles of iron in the following reaction 4fe + 3o2- 2fe2o3
Solution:Balanced chemical equation:4Fe + 3O2 → 2Fe2O3According to stoichiometry: 4 mol of iron (Fe) produces 2 mol of iron(III) oxide (Fe2O3)Thus, 0.030 mol of iron (Fe) produces:(0.030 mol Fe) ×...
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consider the following reaction :2Al + Cr2O3 = Al2O3 +2cr. what is the mass of Al2O3 that will be produced upon complete reaction of 1.20* 10^21 atoms of Al
2Al + Cr2O3 = Al2O3 +2 Сr1 mole of matter cntains 6.022×1023 elementary entities.1.20x1021 atoms of Al equals to 1.20x1021/ 6.022×1023 = 0.2x10-2 moles.According to the equation, n (Al2O3) =...
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Ionic equations for the following
4Li(s) + O2(g) → 2Li2O(s)
2Li (s) + 2H2O (l) 2LiOH (aq) +H2 (g)
Ca(s) + 2H20(g) Ca(OH)2(aq) + H2(g)
2Ca(s) + O2 (g) 2CaO (s)
4Al(s) + 3O2(g) → 2Al2O3(s)
4Li(s) + O2(g) → 2Li2O(s) 2Li (s) + 2H2O (l) → 2Li+(aq) + 2OH-(aq) + H2(g) Ca(s) + 2H2O(l) → Ca2+(aq) + 2OH-(aq) + H2(g) *Usually Ca(OH)2 is almost insoluble...
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When heated, KClO3
decomposes into KCl
and O2.
2KClO3⟶2KCl+3O2
If this reaction produced 77.8 g KCl,
how many grams of O2
were produced?
Solution.n(KCl) = 77.8/74.5 = 1.044 mole = n(KClO3)1.044/2 = x/3 x = n(O2) = 1.566 molesm(O2) = 1.566 * 32 = 50.112 gAnswer. 50.112 g
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When heated, KClO3
decomposes into KCl
and O2.
2KClO3⟶2KCl+3O2
If this reaction produced 62.3 g KCl,
how many grams of O2
were produced?
Mass= Moles * Molecular weightMoles of KCl -> 62.3/74.5 = 0.84 molesMoles of KClO3=Moles of KCl (2KClO3⟶2KCl)Moles of KClO3=0.84 moles2KClO3⟶3O2 1 mole of KClO3 = 3/2 mole of O20.84 mole...
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How many moles of H2O are produced from 0.100 mole of C2H5OH shown in the reaction? C2H5OH + 3O2 2CO2 + 3H2O
According to the equation we obtain 3 molecules of H2O from each molecule of C2H5OH. Thus, from 0.100 mole of C2H5OH we will obtain 0.300 mole of H2O.
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