how many grams of lithium hydroxide are needed to remove 4500 grams carbon dioxide by a submarine atmospheric regulator and acts according to the following formula? 2LiOh+CO2>Li2CO3+H2O
Also how many grams CO2 removed?
If you want to be a nurse, please learn to follow directions. Your School Subject appears to be Chemistry.
convert the 4500 grams of CO2 to moles of CO2.
moles CO2=4500/44
Now, your balanced equation says you need twice that number of moles of LiOH.
molesLiOH= 2*4500/44
Now convert that number of moles of LiOH to grams of LiOH
To determine the number of grams of lithium hydroxide (LiOH) needed to remove 4500 grams of carbon dioxide (CO2), we need to consider the stoichiometry of the balanced chemical equation given:
2LiOH + CO2 -> Li2CO3 + H2O
The coefficients in front of the reactants and products indicate the ratio of moles between them. Therefore, we need to calculate the molar masses of LiOH and CO2 to convert the grams to moles and use the stoichiometric ratio to find the grams of LiOH.
1. Calculate the molar mass of LiOH:
Li = 6.94 g/mol
O = 16.00 g/mol
H = 1.01 g/mol
Molar mass of LiOH = (6.94 g/mol) + (16.00 g/mol) + (1.01 g/mol) = 23.95 g/mol
2. Calculate the molar mass of CO2:
C = 12.01 g/mol
O = 16.00 g/mol (two oxygen atoms)
Molar mass of CO2 = (12.01 g/mol) + (16.00 g/mol) + (16.00 g/mol) = 44.01 g/mol
3. Convert 4500 grams of CO2 to moles:
Moles of CO2 = (4500 g) / (44.01 g/mol)
4. Use the stoichiometric ratio:
From the balanced equation, we can see that 2 moles of LiOH react with 1 mole of CO2. So the conversion factor is 2 moles LiOH / 1 mole CO2.
Moles of LiOH = (Moles of CO2) * (2 moles LiOH / 1 mole CO2)
5. Calculate the grams of LiOH:
Grams of LiOH = (Moles of LiOH) * (Molar mass of LiOH)
By following these steps and plugging in the values, you can determine the number of grams of LiOH needed to remove 4500 grams of CO2.