In the balanced equation MnO2 + 4HCl = MnCl4 +2H2O, how many moles of MnCl2 will be produced when 1.25 mol of H2O are formed?
To find out the number of moles of MnCl2 produced when 1.25 mol of H2O is formed, we can start by determining the mole ratio between MnO2 and MnCl2 using the balanced equation.
The balanced equation is:
MnO2 + 4HCl = MnCl4 + 2H2O
From the equation, we can see that for every 1 mol of MnO2, 1 mol of MnCl4 and 2 mol of H2O are produced. Therefore, the mole ratio between MnO2 and MnCl4 is 1:1, and the mole ratio between MnO2 and H2O is 1:2.
Since 1.25 mol of H2O is formed, we need to determine the number of moles of MnCl2 produced. Since the mole ratio between MnO2 and H2O is 1:2, the number of moles of MnO2 is half of the number of moles of H2O.
Number of moles of MnO2 = 1.25 mol H2O / 2 = 0.625 mol
Since the mole ratio between MnO2 and MnCl2 is 1:1, the number of moles of MnCl2 is equal to the number of moles of MnO2.
Number of moles of MnCl2 = 0.625 mol
Therefore, when 1.25 mol of H2O is formed, 0.625 mol of MnCl2 will be produced.
To determine the number of moles of MnCl2 produced when 1.25 mol of H2O are formed, we first need to identify the stoichiometric coefficients in the balanced equation.
In the balanced equation MnO2 + 4HCl = MnCl4 + 2H2O, the stoichiometric coefficient (the number in front of each compound) indicates the ratio of moles between the reacting compounds.
According to the equation, for every 1 mole of MnO2, 4 moles of HCl, 1 mole of MnCl4, and 2 moles of H2O are produced.
Since you have 1.25 mol of H2O, we need to find the corresponding moles of MnCl2. Given that the ratio of H2O to MnCl2 is 2:1, we can use the ratio to find the moles of MnCl2.
1. First, we determine the moles of H2O using the equation: Moles = Mass / Molar mass.
Assuming the molar mass of H2O is 18.015 g/mol, the mass of 1.25 mol of H2O is:
Mass of H2O = 1.25 mol * 18.015 g/mol = 22.51 g.
2. Next, we can use the stoichiometric ratio to find the moles of MnCl2.
Since the ratio of H2O to MnCl2 is 2:1, we divide the moles of H2O (1.25 mol) by 2 to find the moles of MnCl2 produced:
Moles of MnCl2 = 1.25 mol H2O / 2 = 0.625 mol MnCl2.
Therefore, when 1.25 mol of H2O are formed, 0.625 mol of MnCl2 will be produced according to the balanced equation.