In the reaction between zinc and sulfuric acid, how many grams of sulfuric acid are required to produce 1.0 grams Hydrogen.
A
1.0
B
2.0
C
49
D
98
Here is a worked example of a stoichiometry problem. This will work 99.9% of them for you.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine how many grams of sulfuric acid are required to produce 1.0 gram of hydrogen, we need to use stoichiometry to convert between the given substances.
First, let's write the balanced chemical equation for the reaction between zinc (Zn) and sulfuric acid (H2SO4):
Zn + H2SO4 -> ZnSO4 + H2
According to the equation, for every 1 mole of zinc (65.38 g), we need 1 mole of sulfuric acid (98.09 g) to produce 1 mole of hydrogen gas (2.02 g).
Now, we can set up a proportion to solve for the mass of sulfuric acid required:
(1.0 g H2) / (2.02 g H2) = (x g H2SO4) / (98.09 g H2SO4)
Cross-multiplying and solving for x, we get:
x = (1.0 g H2SO4) * (98.09 g H2SO4) / (2.02 g H2)
x ≈ 48.51 g H2SO4
Therefore, the closest answer choice is C) 49 grams.