An engineer is trying to produce as much hydrogen gas as the company can using the equipment they have.
The engineering obtained the following data from research.
Sodium + Sulfuric Acid
Sodium Sulfate + Hydrogen
Mass of Na (g)
Mass of H,SO. (g)
Mass of Na,so ()
Mass of H. (g)
1149.5
2450
3549.5
50
2299
4900
7099
100
3448.5
1
7350
10648.5
150
Beginning: (5 points)
Reacting 2299 g of sodium requires 4900 g of sulfuric acid, as seen in the data table. How many moles of each substance is
this? Show your work and/or explain the math that you used to arrive at this answer.
Developing: (5 points).
Based on the chemical equation, how much sulfuric acid, in grams, is consumed from the reaction of 1450 g of sodium
metal? Show your work and/or explain the math that you used to arrive at this answer.
Proficient: (6 points)
The equipment the engineer has can only hold a maximum of 1450 g of sodium before it is mixed with excess sulfuric acid
to carry out the reaction described above. How much hydrogen gas can be produced from the equipment they currently
have? Show your work and/or explain the math that you used to arrive at this answer.