PERIOD 1
(Kelly)
1. A 2.00 g sample of ammonia is mixed with 4.00 g of oxygen. Reactants: 4 NH3+ 5 O2 Products: 4
NO+ 6 H2O Which element is the limiting reactant?
2. What is the molar mass of sodium carbonate?
(Ali)
3. Calculate how many grams are in 4.34 moles of Sodium Carbonate.
4. If 15 grams of copper (II) Chloride reacts with 20 grams of sodium nitrate, how much sodium
chloride can be formed?
(Madeleine)
5. Write the formulas for: Potassium Peroxide, Cadmium (II) Hypochlorite
6. Name: NH4Cl, Al(NO2)3
7. Using the balanced equation of __C6H10 + __O2  __CO2 + __H2O, how much of the excess
reactant is left if one has 35g hexacarbon decahydride and 45g oxygen?
(Sienna)
8. What is the mass of 4.00 moles of Cu(CN)2 ?
9. Balance: __Al203  __Al + __02
(Joe)
10. Balance: CH5N + O2  C02 + H2O + NO2
11. Calculate the molar mass of Fe3(PO4)2
(Cory)
12. Sodium hydroxide reacts with sulfuric acid (H2SO4) to form water and sodium sulfate. How many
grams of water will be formed if you start with 3.75 moles of sodium hydroxide?
(Anastasia)
13. If I do this combustion reaction with 35 grams of C6H10 and 45 grams of oxygen, how many grams
of carbon dioxide will be formed?
14. What is the limiting reagent in the previous problem?
(Clarissa)
15. Find the Molar Mass of copper (II) sulfate
16. Find the molar mass of Ag(NO3)2
(Yulee)
17. Equation: 2 Mn + 3 F2  2 MnF3 If 3.70 mol Mn reacts with F2, how many moles of MnF3 will
form?
18. In a gaseous reaction, hydrogen sulfide (common name for dihydrogen sulfide) burns in oxygen
to form sulfur dioxide and water vapor. How many grams of oxygen will react with 3.22 g
hydrogen sulfide?
(Rachel)
19. __Fe+__Cl2  __FeCl3
20. __Ca(OH)2 +__CO2 __CaCO2+__H2O
(Heidi)
21. Carbon disulfide and oxygen react to form carbon dioxide and sulfur dioxide, If 20.0g of each
reactant are present,
a. Balance the equation
b. Limiting reactant
c. Moles of sulfur dioxide formed
22. Rubidium nitrate and beryllium fluoride react to form beryllium nitrate and rubidium fluoride. There
are 10.5 g rubidium nitrate and 48.0g beryllium fluoride.
A. Balance equation
B. limiting reactant
C. Mass of rubidium fluoride produced
(Aria)
23. How many moles of carbon diozide form when 21.07g of methane (CH4) burn?
24. A strip of zinc metal with a mass of 2.00g is placed in a solution containing 2.50g of silver (I)
nitrate, causing a single replacement reaction. How many moles of the excess reactant will be left
at the end of the reaction?
(Adrian)
25. Find the molar mass of the compounds :
a. (NH4)2CO3
b. Zn(C2H3O2)2
26. Balance the equation: ___ GaBr3+ ___ Na2SO3 ___ Ga2(SO3)3 + ___ NaBr
(Cierra)
27. When copper (II) chloride reacts with sodium nitrate, copper (II) nitrate an sodium chloride are
formed
a. write the balanced equation
b. if 15 g of copper (II) chloride react with 20 g of sodium nitrate l, how much sodium
chloride can be formed?
c. what is the limiting reactant?
d. how much excess is left?
(Lily)
28. *3.0 moles of Fe and 5.0 moles of O react to form iron oxide*
a. What is the limiting reactant?
b. How many moles will each product form?
c. How many moles of the excess reactant will remain after the reaction is complete?
(Jamie)
29. Using the Hoffman apparatus for electrolysis, a chemist decomposes 36g of water into its
gaseous elements. How many grams of hydrogen gas should be produced?
30. A strip of zinc metal with a mass of 2.00 g is placed in a solution containing 2.50g of silver (I)
nitrate, causing a single replacement reaction.
a.) Balanced chemical equation
b.) which reactant is limiting
c.) How many grams of Ag will form?
d.) How many grams of Zn(NO3)2 will form?
e.) How many moles of the excess reactant will be left at the end of the reaction?