| Chemistry: Stoichiometry |
|
2 NaOH + H2SO4 --> 2 H2O + Na2SO4
|
|
Compound
|
Molar Masses (g/mole)
|
|
NaOH
|
40.0
|
|
H2SO4
|
98.1
|
|
H2O
|
18.0
|
|
Na2SO4
|
142
|
Example:
If the reaction starts with 50.0g of NaOH, how many grams of Na2SO4 will form?
Solution:
|
|
|
General Questions |
|
|
|
| If the reaction consumes 100 g of NaOH, how many grams of Na2SO4 should form? |
| If 475 g of H2O form, predict how many grams of NaOH must have been consumed? |
| The reaction generates 35.0 g of Na2SO4. How many grams of H2SO4 should have been used up? |
| If 25.0 g of NaOH is used, how many grams of H2SO4 should react? |
|
Question Group #2 |
|
Directions and/or Common Information: A reaction produces 100 g of H2O. |
|
| How many grams of NaOH will be consumed? |
| How many grams of H2SO4 will be consumed? |
| If the law of conservation of mass holds true, the total mass of the reactants (NaOH and H2SO4) should equal the total mass of the products (H2O and Na2SO4). Without doing a stoichiometry problem, predict how many grams of Na2SO4 should form. |
|
|
|
|
E Saylor
|
|
Show Related AlgebraLab Documents
|
|