1.how many mole, Fe can be made from Fe2O3 by the use of 20 moles of carbon monoxide, CO in the following reaction?
Fe2O3+ 3CO = 2Fe+ 3CO2
2. How manhy moles of H2O are produced when 2.75 moles of O2 are consumed if burning methyl alcohol, CH3OH, according to the following equation?
2CH3OH +3O2 = 2CO2 +4H2O
anyone?
To answer these questions, we need to use stoichiometry: the quantitative relationship between substances in a chemical reaction. The coefficients in the balanced equation represent the ratio of moles of reactants and products.
1. To determine how many moles of Fe can be made from Fe2O3, we need to use the mole ratio between Fe2O3 and Fe. From the balanced equation, we can see that 1 mole of Fe2O3 produces 2 moles of Fe. Therefore, for every 1 mole of Fe2O3, 2 moles of Fe are formed.
Given that we have 20 moles of CO, we need to determine how many moles of Fe2O3 are needed to react with 20 moles of CO. From the balanced equation, we can see that the molar ratio between CO and Fe2O3 is 3:1. Therefore, for every 3 moles of CO, we need 1 mole of Fe2O3.
Using this information, we can set up a proportion:
3 moles CO / 1 mole Fe2O3 = 20 moles CO / x moles Fe2O3
Cross-multiplying and solving for x, we get:
x = (20 moles CO)(1 mole Fe2O3) / (3 moles CO) = 20/3 ≈ 6.67 moles Fe2O3
So, 6.67 moles of Fe2O3 are needed to produce the maximum amount of Fe with 20 moles of CO.
2. Similarly, to determine the number of moles of H2O produced, we need to use the mole ratio between O2 and H2O. From the balanced equation, we can see that 3 moles of O2 react to produce 4 moles of H2O.
Given that we have 2.75 moles of O2, we can calculate the moles of H2O using the mole ratio:
(2.75 moles O2) / (3 moles O2) * (4 moles H2O) = 3.67 moles H2O
Therefore, 3.67 moles of H2O are produced when 2.75 moles of O2 are consumed in the reaction.