Most metals are very reactive, as are the elements in the halogen group. aluminum, for instance, for example, reacts with elemental chlorine to form aluminum chloride. if you have a 13.5 g sample of al, which choice below is true?
a. you will need 23.6 g cl2 for complete reaction and will produce 66.7 g of alcl3.
b. you will need 53.2 g cl2 for complete reaction and will produce 66.7 g of alcl3.
c. you will need 11.8 g cl2 for complete reaction and will produce 49.0 g of alcl3.
d. you will need 26.6 g cl2 for complete reaction and will produce 49.0 g of alcl3. reset selection

 B. you will need 53.2 g Cl2 for complete reaction and will produce 66.7 g of AlCl3.

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number of particles.

To calculate the moles, we use the equation:

The balanced reaction is:

2 moles of aluminium react with= 3 moles of chlorine

Thus 0.5 moles of aluminium react with=  moles of chlorine

Mass of chlorine=

2 moles of aluminium produce = 2 moles of aluminium chloride

Thus 0.5 moles of aluminium react with=  moles of aluminium chloride

Mass of aluminium chloride=

Thus 53.2 g of chlorine is used and 66.7 g of  aluminium chloride is produced.

i think it is d. e because the next one is igneous.

"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"