theoretical yield, limiting reactant, excess, and percent yield for
replacement reaction (laboratory)
Find the molar mass of each compound.
3. 0.4 moles of Sn to atoms
4. 32 g of K2O to molecules
5. 3.7 g of H2 to moles
6. 800 g of CaCl2 to moles
7. 0.75 moles of H2O to grams
8. 9.0 g of Cl2 to atoms
9. 0.5 moles of KNO3 to grams
Find the percent composition for each element in the compound.
12. MgO + H2O -----> Mg(OH)2
If you started with 3.7 moles of magnesium oxide, how many moles of magnesium hydroxide would be produced?
13. Na + I2 ---> NaI
If 2.8 grams of sodium were used for the reaction, and an excess of iodine was present, how many moles of sodium iodide would be produced?
14. N2 + 3 H2 ------> 2 NH3
How many grams of ammonia were produced if you started with 10 moles of nitrogen and excess hydrogen gas?
15. Pb(NO3)2 + K2CrO4 --> PbCrO4 + 2 KNO3
If you started with 0.97 g of K2CrO4 and excess Pb(NO3)2, how many grams of KNO3 could be produced?
16. Pb(NO3)2 + K2CrO4 --> PbCrO4+ 2 KNO3
If you started with 0.97 g of K2CrO4 and 0.97g Pb(NO3)2, how many grams of KNO3 could be produced? How many grams of PbCrO4 could be produced? How much of the left over reactant will be present at the end of the reaction?