Which of the following would result in the magnesium ribbon 'dissappearing' in less than 45 seconds? *Warming the acid
*Using 2g magnesium ribbon
*Stirring the mixture
*Adding water to the acid

BTW:- The acid is sulfuric acid

your should probably be warming the acid

Explanation:

because when you are it is disappearing

Warming the acid

Explanation:

This is because when the acid is heated, the particle of the acid gain more energy (kinetic to be more precise) causing more collisions to occur, colliding even more with the particles of the magnesium ribbon. This increases the rate of disappearance of the magnesium ribbon.

"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"

with this one i know the answer in craters one reason i looked it up and i learned about it there is my evidence