For the reaction
CH4+ 2 O2 → CO2+ 2 H2O ,
what is the maximum amount of CO2
(44.0095 g/mol) which could be formed from
15.3 g of CH4 (16.0425 g/mol) and 6.2 g of O2
(31.9988 g/mol)?
Answer in units of g
You must determine the limiting reactant. In the equation CH4 and O2 are in a 1:2 ratio. Compare this to the ratio of the masses of the reactants given. Find the number of moles of CH4 and O2 and then find their ratio. If, for example, CH4 was 1 and O2 1.5 (1:1.5), O2 would be the limiting reagent. Then use the limiting reagent through stoichiometry to find the max amount of CO2
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To find the maximum amount of CO2 that could be formed, we need to determine the limiting reactant. The limiting reactant is the reactant that is completely consumed first and determines the amount of product that can be formed.
First, we need to convert the given masses of CH4 and O2 into moles using their molar masses:
Molar mass of CH4 (methane) = 16.0425 g/mol
15.3 g CH4 * (1 mol / 16.0425 g) = 0.954 mol CH4
Molar mass of O2 (oxygen) = 31.9988 g/mol
6.2 g O2 * (1 mol / 31.9988 g) = 0.1938 mol O2
Now, we need to determine the stoichiometric ratio between CH4 and CO2. From the balanced equation, we can see that one mole of CH4 reacts to produce one mole of CO2.
So, in this reaction, the moles of CO2 formed will be equal to the moles of CH4.
Since 0.954 mol CH4 is the smaller amount compared to 0.1938 mol O2, CH4 is the limiting reactant.
To calculate the maximum amount of CO2 that can be formed, we can use the moles of CH4:
0.954 mol CH4 * (1 mol CO2 / 1 mol CH4) = 0.954 mol CO2
Finally, we can convert the moles of CO2 to grams using its molar mass:
0.954 mol CO2 * 44.0095 g/mol = 41.98 g CO2 (rounded to two decimal places)
Therefore, the maximum amount of CO2 that can be formed from 15.3 g of CH4 and 6.2 g of O2 is approximately 41.98 grams.
To find the maximum amount of CO2 that can be formed, we need to determine the limiting reactant in the reaction. The limiting reactant is the reactant that is completely consumed and determines the maximum amount of product that can be formed.
First, we need to calculate the number of moles for each reactant using their respective molar masses:
Molar mass of CH4 = 16.0425 g/mol
Number of moles of CH4 = Mass of CH4 / Molar mass of CH4
= 15.3 g / 16.0425 g/mol
Molar mass of O2 = 31.9988 g/mol
Number of moles of O2 = Mass of O2 / Molar mass of O2
= 6.2 g / 31.9988 g/mol
Using the balanced equation: CH4 + 2 O2 → CO2 + 2 H2O, we can determine the stoichiometric ratio between CH4 and CO2. The ratio is 1:1, which means for every 1 mole of CH4, we get 1 mole of CO2.
However, the ratio between O2 and CO2 is 2:1, which means for every 2 moles of O2, we get 1 mole of CO2.
Now, we need to compare the calculated number of moles of CH4 and O2 to determine the limiting reactant. The reactant with the smaller number of moles is the limiting reactant.
Number of moles of CH4 = 15.3 g / 16.0425 g/mol ≈ 0.9531 mol
Number of moles of O2 = 6.2 g / 31.9988 g/mol ≈ 0.1938 mol
Since O2 has fewer moles than CH4, it is the limiting reactant.
Now, we can calculate the maximum amount of CO2 that can be formed by using the stoichiometric ratio between O2 and CO2.
From the balanced equation: CH4 + 2 O2 → CO2 + 2 H2O
We can see that 2 moles of O2 produce 1 mole of CO2.
Number of moles of CO2 = (0.1938 mol O2) * (1 mol CO2 / 2 mol O2)
= 0.0969 mol CO2
Finally, we can calculate the mass of CO2 using the molar mass:
Mass of CO2 = (Number of moles of CO2) * (Molar mass of CO2)
= 0.0969 mol * 44.0095 g/mol
≈ 4.26 g
Therefore, the maximum amount of CO2 that could be formed from 15.3 g of CH4 and 6.2 g of O2 is approximately 4.26 g.