How many moles of h2o will be produced from 42.0g of h2o2? i need the equations for what to do because i am not sure how to do it.

Hey there!

Molar mass:

H2O2 = 34,01 g/mol

H2O = 18,01 g/mol

By the stoichiometry of the reaction:

2 H2O2 = 2 H2O + O2

2 * 34,01 g H2O2 2 * 18,01 g H2O

42,0 g H2O2 m

m = ( 42,0 * 2 * 18,01 ) / ( 2 * 34,01 )

m = 1512,84 / 68,02

m = 22,24 g H2O

Therefore:

1 mole H2O 18,01 g

?? moles H2O 22,24 g

moles H2O = 22,24 * 1 / 18,01

moles H2O = 22,24 / 18,01

moles H2O = 1,23 moles

Hope this helps!

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"