The answer is 10 moles of carbon monoxide.
2 C + O2 = 2 CO
CO is form in high temperatures. 10 moles will form by 5 O2 moles.
The reaction is:2 C + O2 = 2 COSo 2,1 moles are obtained.
The reaction is:2 C + O2 = 2 CO1,7 moles of carbon monoxide are obtained.
Balanced equation. 2S + 3O2 --> 2SO3 1.32 moles O2 (2 moles SO3/3 moles O2) = 0.880 moles sulfur trioxide produced ========================
The thermal decomposition reaction is:2 KO2------------K2O2 + O20,2 moles of O2 are produced from o,4 moles KO2.
This is a chemical calculation. 2.5 moles will C reacting with O2.
The burning reaction is:C + O2 = CO2For 6 moles oxygen the equivalent is 6 moles carbon.
The reaction is:2 KClO3 = 2 KCl + 3 O2 (three moles of oxygen)
The answer is o,5 moles MgO.
2Al + 3O2 --> 2Al2O3 0.78 moles O2 (2 moles Al2O3/3 moles O2) 0.52 moles Al2O3 produced ===========================( assuming oxygen limits )
5 moles RbNO3 (3 moles O2/2 moles RbNO3) = 7.5 moles oxygen gas produced
2 moles of Na2O are produced. 4 moles of Na react with 1 mole of O.
15 moles of O2 are produced by the decomposition if 10 moles potassium chlorate 2 KClO3 and 2 KCl plus 3O2.
Potassium chlorate = KClO3Decompostion: 2KClO3 ==> 3O2 + 2KCl7.5 moles KClO3 x 3 mole O2/2 moles KClO3 = 11.25 moles O2
The reaction is:2 KClO3 = 2 KCl + 3 O238,4 moles of oxygen are produced.
Balanced equation first. 4P + 5O2 -> 2P2O5 8.00 mole O2 (2 mole P2O5/5 mole O2) = 3.20 moles P2O5 produced
2Ca + O2 --> 2CaO 0.016 moles O2 (2 mole CaO/1 mole O2) = 0.032 moles calcium oxide produced ========================
5C +5O2 ----> 5CO2 So 5 moles of carbon dioxide are produced from 5 moles of oxygen - if there is plenty of carbon and it is not the limiting ingredient.
2KClO3 --> 2KCl + 3O2For every 3 moles of oxygen gas produced, 2 moles of potassium chlorate are used.6 moles O2 * (2 moles KClO3 reacted / 3 moles O2 produced) = 4 moles KClO3
First you need to find the balanced reaction:2S + 3O2 --> 2SO3So using the balanced reaction we see that for every 3 moles of oxygen consumed, 2 moles of sulfur trioxide are produced:1.2 moles O2 consumed * (2 moles SO3/3 moles O2) = 0.8 mole of SO3 produced
2H2 + O2 -> 2H2O Therefore, 12.0 moles of water.
Assuming the reaction is S + O2 --> SO2, this equation is balanced as written, with everything in a 1:1 molar ratio. So, 67.1 moles of product would require 67.1 moles of O2 reactant.
The answer is 4,09 moles.
To determine the number of moles of Fe that can be made from 25 moles of Fe2O3, you need to write the balanced chemical equation for producing O2 from Fe2O3. 2Fe2O3 = 4Fe + 3O2, which means that 2 moles of Fe2O3 will produce 4 moles of Fe and 3 moles of O2 . Set up a proportion. 3 moles of O2 ÷ 2 moles of Fe2O3 = x moles of O2 ÷ 25 moles of Fe2O3 Cross multiply and divide. 3 moles of O2 * 25 moles of Fe2O3 ÷ 2 moles of Fe2O3 = 37.5 moles of O2 produced.
5 moles:10 Na + (enough) O2 --> 5 Na2O
The total number of moles of NO produced when 1,0 mole of O2 is completely consumed is 2.
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