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Chemistry 10 Advanced term two revision

Q1: 2KClO3(s)
2KCl + 3O2
How many conversions factor mole to mole factors can we make?
Q2: How many moles of hydrogen are needed to produce 5.0 moles of water?
2H2 + O2
Q3: How many moles of CO2 will Produce from burning 100 g of methane?
CH4 + 2O2
CO2 + 2H2O
(C=12g/mol, O=16 g/mol)
Q4: How many grams of oxygen are needed to react with 2.00 moles of Mg?
2Mg + O2
(Mg= 14 g/mol, O = 16 g/mol)
Q5: Some antacid tablets contain aluminum hydroxide. The aluminum hydroxide reacts with stomach acid
according to the equation:
Al(OH )3+ 3HCl → AlCl3+ 3H2O.
Determine the moles of acid neutralized if a tablet contains 0.200 mol of Al (OH )3
Q6: A 54.0-g sample of aluminum reacts with 508 g of iodine according to this equation:
2Al + 3I2→ 2AlI3.
a) Find the number of moles of each reactant. 2.00 mol Al, 2.00 mol I2
b) which is the limiting reactant: I2
c)how many moles of AlI3 are formed: 1.33 mol
Q7: What is the balanced equation for the reaction between KOH and CuSO4?
2KOH (aq) + CuSO4(aq) → Cu (OH)2(s) +K2SO4(aq)
Q8: a) If 25.0 g of zinc is in a sample of bronze,determine the theoretical yield of hydrogen gas. 0.771 g of H2 is the theoretical yield
Zn + 2HCl → H2+ ZnCl2
(Zn=65.38 g/mol, H = 1 g/mol)
b. If the reaction yields 0.680 g H2, determine the percent yield 88.2% yield of H2
Q9: CH4+ 2O2→ CO2 + 2H2O.
determine the percent yield if 10.0 g of methane (16 g/mol) is burned producing 19.5 g of water. 86.7% yield
Q10: depicts an equation with squares representing Element M and circles representing Element N.
Write a balanced equation to represent the picture shown, using the smallest whole-number ratios. Write mole ratios for this equation.
2M2N → M4 + N2
1 mol N2 / 2mol M2N ( 6 conversion)
Q11: Oxygen Production the Russian Space Agency uses potassium superoxide (KO2) for the chemical
oxygen generators in their spacesuits.
4KO2+ 2H2O + 4CO2→ 4KHCO3+ 3O2 ( H2O =18 g/mol, CO2 = 44 g/mol , KO2 = 71 g/mol)
If the mass of oxygen is 380 grams. find the mass of KO2, H2O, CO2, KHCO3
mass KO2= 1100 g, mass H2O =140 g, mass CO2 = 7.0 ×102 g, mass KHCO3= 1600 g
Q12: Chloroform (CHCl3), an important solvent, is produced by a reaction between methane and chlorine.
CH4(g) + 3Cl2(g) → CHCl3(g) + 3HCl(g) ( CH4=16, Cl2=71, CHCl3=119.5)
How much CH4, in grams, is needed to produce 50.0 grams of CHCl3 6.72 g CH4
Q13: uses squares to represent Element M and circles to represent Element N.
a. Write the balanced equation for the reaction.
b. If each square represents 1 mol of M and each circle represents 1 mol of N, how many moles of M and N were present at the start of the reaction?
c. How many moles of product form? How many moles of Element M and Element N are unreacted?
d. Identify the limiting reactant and the excess reactant.
a.3M2 + N2
→ 2M3N
b. 6 moles of element M (in the form of 3 moles of M2) and 6 moles of element N (likewise, 3 moles of N2)
c. 2 moles of M3N form with 2 moles of N2 unreacted (4 total moles of element N)
d.M2 is the limiting reactant and N2 is the excess reactant.
Q14: Aqueous potassium iodide (KI) reacts with lead nitrate Pb (NO3)2 in solution. forming solid lead iodide (Write net ionic equation)
Q15: Zinc (Zn) is used as a corrosion-resistant coating on iron and steel. It is also an essential trace element in your diet. Calculate the number of moles of zinc
that contain 4.50 × 1024 atoms? 7.48 mol Zn
Q16: Predict whether the following single-replacement reactions will occur. If a reaction occurs, write a balanced equation for the reaction.
K(s) + ZnCl2(aq) →
Cl2(g) + HF (aq) →
Fe(s) + Na3PO4(aq) →
Al(s) + Pb (NO3)2(aq) →
Fe(s) + CuSO4(aq) →