For the reaction Ba(OH)2+2HCLO3 -> Ba(CIO3)2+2H2O calculate the no. of mole of H2O formed .when .01 mole of Ba(OH)2 is treated with 0.0250 moles of HCLO3
To find the number of moles of H2O formed, we can use the stoichiometry of the balanced chemical equation.
The balanced chemical equation is:
Ba(OH)2 + 2HClO3 -> Ba(ClO3)2 + 2H2O
From the equation, we can see that for every 1 mole of Ba(OH)2, 2 moles of H2O are formed.
Given:
Moles of Ba(OH)2 = 0.01 mol
Moles of HClO3 = 0.0250 mol
Since the mole ratio of Ba(OH)2 to H2O is 1:2, we can calculate the moles of H2O formed using the given moles of Ba(OH)2:
Moles of H2O = 2 * Moles of Ba(OH)2
Moles of H2O = 2 * 0.01 mol
Moles of H2O = 0.02 mol
Therefore, when 0.01 mole of Ba(OH)2 is treated with 0.0250 moles of HClO3, 0.02 moles of H2O are formed.
To calculate the number of moles of H2O formed in the reaction, we need to use the balanced chemical equation and the stoichiometry of the reaction.
The balanced chemical equation for the reaction is:
Ba(OH)2 + 2HClO3 -> Ba(ClO3)2 + 2H2O
According to the stoichiometry of the reaction, for every 1 mole of Ba(OH)2, 2 moles of H2O are formed.
In this case, we have 0.01 moles of Ba(OH)2 and 0.0250 moles of HClO3.
From the stoichiometry, we know that for every 0.01 moles of Ba(OH)2, 0.02 moles of H2O are formed (because the ratio of Ba(OH)2 to H2O is 1:2).
Therefore, when 0.01 moles of Ba(OH)2 is treated with 0.0250 moles of HClO3, the number of moles of H2O formed is 0.02 moles.
So, the answer is 0.02 moles of H2O formed.
0.44
0.01 mol Ba(OH)2 will produce 0.02 mole H2O if all of the HClO3 needed is present for the reaction.
0.0250 HClO3 will produce 0.025 mole H2O if all of the Ba(OH)2 needed is present for the reaction.
So which is the limiting reagent? Which amount of H2O will be produced?