How many molecules of (CH3)2NH are needed to react completely with 2.00mg of H2C2O4? Help i don't understand this process!
(CH3)2NH is a base(monoacidic)
H2C2O4 is an acid(dibasic)
2(CH3)2NH + H2C2O4 ==> 2(CH3)2NH2^+ + C2O4^-
How many moles H2C2O4 do you have? That is g/molar mass = 0.002g/molar mass H2C2O4 = ? moles.
If 1 mol H2C2O4 contains 6.02E23 molecules, then ? moles has how many molecules.
Look at the equation. It takes twice as many molecules of (CH3)2NH.
To determine the number of molecules of (CH3)2NH needed to react completely with 2.00 mg of H2C2O4, we need to follow a step-by-step process. Here's how:
1. Calculate the molar mass of H2C2O4:
H = 1.01 g/mol (2 Hydrogen atoms)
C = 12.01 g/mol (2 Carbon atoms)
O = 16.00 g/mol (4 Oxygen atoms)
Add all the masses: (2 * 1.01 g/mol) + (2 * 12.01 g/mol) + (4 * 16.00 g/mol) = 90.03 g/mol
2. Convert 2.00 mg of H2C2O4 to moles:
Divide the given mass by the molar mass of H2C2O4:
2.00 mg / 90.03 g/mol = 0.0222 moles
3. Use the balanced chemical equation to determine the molar ratio:
The balanced equation is needed in order to determine the stoichiometry, meaning the ratio of molecules involved in the reaction. For example, if the balanced equation is:
CH3NH2 + H2C2O4 → (CH3)2NH + CO2 + H2O
From the equation, you can see that 1 mole of H2C2O4 reacts with 1 mole of (CH3)2NH.
4. Convert moles of H2C2O4 to moles of (CH3)2NH:
Since the molar ratio is 1:1, the number of moles of (CH3)2NH will be the same as that of H2C2O4, which is 0.0222 moles.
5. Convert moles of (CH3)2NH to molecules:
Multiply the number of moles by Avogadro's number (6.022 x 10^23 molecules/mol):
0.0222 moles * (6.022 x 10^23 molecules/mol) = 1.34 x 10^22 molecules
Therefore, to react completely with 2.00 mg of H2C2O4, you would need approximately 1.34 x 10^22 molecules of (CH3)2NH.