Consider the following balanced equation cac2(s) + 2h2o(i) → ca(oh)2(s) + c2h2(g)
when 1.50 mol of cac2 are allowed to react, how many moles of ca(oh)2 is
produced?

1.50 moles of  CaC₂ will produced 1.50 moles of Ca(OH)₂ .

Explanation:

Given data:

Moles of CaC₂ = 1.50 mol

Moles of Ca(OH)₂ = ?

Solution:

First of all we will write the balanced chemical equation.

CaC₂  + 2H₂O   →  Ca(OH)₂ + C₂H₂

Now we will compare the moles of CaC₂  with Ca(OH)₂ from balanced chemical equation.

                       CaC₂      :       Ca(OH)₂

                        1            :           1

                       1.50       :          1.50

1.50 moles of  CaC₂ will produced 1.50 moles of Ca(OH)₂ .

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.

"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"