Given the following reaction:
4 KO2 + 2 H2O + 4 CO2 4 KHCO3 + 3 O2
How many moles of H2O are needed to react with 12.15 moles of CO2? moles
A chemical reaction occurs between solutions of LiCl and silver nitrate. This reaction produces a precipitate that is recovered, dried and massed. The mass of the precipitate is found to be 14.391074. What is the percent yield of the reaction if 11.4453 grams of LiCl was reacted with excess silver nitrate?
Here is an example of a stoichiometry problem. Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine the moles of H2O needed to react with 12.15 moles of CO2, we can use the balanced chemical equation given:
4 KO2 + 2 H2O + 4 CO2 4 KHCO3 + 3 O2
From the balanced equation, we can see that the ratio between H2O and CO2 is 2:4 or 1:2.
So for every 2 moles of CO2, we need 1 mole of H2O.
To find the moles of H2O needed to react with 12.15 moles of CO2, we can set up a proportion:
(2 moles of CO2) / (1 mole of H2O) = (12.15 moles of CO2) / (x moles of H2O)
Cross-multiplying and solving for x:
2 * x = 12.15
x = 12.15 / 2
x = 6.075 moles
Therefore, 6.075 moles of H2O are needed to react with 12.15 moles of CO2.
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To calculate the percent yield of a reaction, we need to compare the actual yield with the theoretical yield.
In this case, the mass of the precipitate obtained is given as 14.391074 grams.
To determine the theoretical yield, we need to calculate the amount of precipitate that would be produced based on the balanced chemical equation.
From the balanced equation, we can determine the mole ratio between LiCl and the precipitate formed. Let's assume it is a 1:1 ratio.
So if 11.4453 grams of LiCl were reacted and we assume a 1:1 mole ratio, the moles of the precipitate formed would be:
Moles of precipitate = (11.4453 grams of LiCl) / (molar mass of LiCl)
Next, we can convert the moles of the precipitate to grams using the molar mass of the precipitate:
Mass of the precipitate = (moles of the precipitate) * (molar mass of the precipitate)
Finally, we can calculate the percent yield using the formula:
Percent yield = (actual yield / theoretical yield) * 100
The actual yield is given as 14.391074 grams, and the theoretical yield is calculated as explained above.
Percent yield = (14.391074 grams / theoretical yield) * 100