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VocabularyMole to mole Limiting Reactants Mass to mass Mass to Mole Percent Yield

Stoichiometry A 100

The calculation of quantities in chemical reactions A 100

Limiting reactant A 200

Reactant that runs out first A 200

Theoretical yield A 300

Predicted amount of product A 300

Excess reactant A 400

Reactant that remains when reaction ends A 400

Actual yield A 500

Amount of product that is recovered A 500

The rusting of iron is represented by the equation 4Fe + 3O 2  2Fe 2 O 3. If you have a 1.50 mol sample of iron, how many moles of Fe 2 O 3 will there be after the iron has rusted completely? B 100

0.75 mol Fe 2 O 3 B 100

For the reaction C 2 H 4 (g) + 3O 2 (g)  2CO 2 (g) + 2H 2 O(g); if 6.0 mol of CO 2 are produced, how many moles of O 2 were reacted? B 200

9.0 mol O 2 B 200

A 3.0 mol sample of KClO 3 was decomposed according to the equation 2KClO 3 (s)  2KCl(s) + 3O 2 (g); How many moles of O 2 are formed? B 300

4.5 mol O 2 B 300

How many moles of ammonia will be required to produce 10.0 mol of water based on the following equation: 4NH 3 (g) + 7O 2 (g)  4NO 2 (g) + 6H 2 O(g) B 400

6.67 mol NH 3 B 400

An excess of Al and 6.0 mol of Br 2 are reacted according to the equation 2Al + 3Br 2  2AlBr 3 ; How many moles of AlBr 3 will be formed? B 500

4.0 mol AlBr 3 B 500

For the reaction 2S(s) + 3O 2 (g) → 2SO 3 (g) if 6.3 g of S is reacted with 10.0 g of O 2, which one will be the limiting reactant. C 100

S is the limiting reactant C 100

For the reaction 2Cl 2 (g) + 4NaOH(aq) → 3NaCl(aq) + NaClO 2 (aq) + 2H 2 O(l) 11.9 g Cl 2 is reacted with 12.0 g NaOH. Determine which is the limiting reactant. C 200

NaOH is the limiting reactant C 200

Consider the reaction Mg 2 Si(s) + 4H 2 O(l) → 2Mg(OH) 2 (aq) + SiH 4 (g) Which of the reactants is in excess if we start with 50.0 g of each reactant? C 300

H 2 O is in excess C 300

DAILY DOUBLE C 400 DAILY DOUBLE Place A Wager

Sodium and water react according to the reaction 2Na(s) + 2H 2 O(l) → 2NaOH(aq) + H 2 (g) What number of moles of H 2 will be produced when 4 mol Na is added to 2 mol H 2 O? C 400

1 mol H 2 C 400

CaCO 3 (s) + 2HCl(aq) → CaCl 2 (aq) + CO 2 (g) + H 2 O(l) 68.1 g solid CaCO 3 is mixed with 51.6 g HCl. What number of grams of CO 2 will be produced? C 500

15.0 g CO 2 C 500

For the reaction 2Cl 2 (g) + 4NaOH(aq)  3NaCl(aq) + NaClO 2 (aq) + 2H 2 O(l) How many grams of NaCl can be produced from 10.9 g of Cl 2 and excess NaOH? D 100

13.5 g NaCl D 100

Consider the reaction Mg 2 Si(s) + 2H 2 O(l) → 2Mg(OH) 2 (aq) + SiH 4 (g) Calculate the number of grams of silane gas, SiH 4, formed if 25.0 g of Mg 2 Si reacts with excess H 2 O. D 200

10.5 g SiH 4 D 200

Fe 3 O 4 reacts with CO according to the reaction Fe 3 O 4 (s) + 4CO(g) → 4CO 2 (g) + 3Fe(s) If 201 g Fe 3 O 4 is reacted with excess CO, what mass of CO 2 will be produced? D 300

153 g CO 2 D 300

Consider the reaction 2CH 4 (g) + 3O 2 (g) + 2NH 3 (g) → 2HCN(g) + 6H 2 O(g) If 128 g NH 3 is reacted with excess CH 4 and O 2, what mass of HCN can be produced? D 400

203 g HCN D 400

Calculate the mass of carbon dioxide produced from 11.2 g of octane, C 8 H 18, in the following reaction. 2C 8 H 18 (g) + 25O 2 (g) → 16CO 2 (g) + 18H 2 O(g) D 500

34.5 g CO 2 D 500

How many moles of oxygen are produced by decomposing 41.1 g of H 2 O 2 according to the equation 2H 2 O 2 (l) → 2H 2 O(l) + O 2 (g) E 100

0.604 mol O 2 E 100

How many moles of O 2 are required for the complete reaction of 45 g of C 2 H 4 to form CO 2 and H 2 O? E 200

4.8 mol O 2 E 200

For the reaction 2Cl 2 (g) + 4NaOH(aq) → 3NaCl(aq) + NaClO 2 (aq) + 2H 2 O(l) how many moles of Cl 2 are needed to react with 14.4 g NaOH? E 300

0.180 mol Cl 2 E 300

Fe 2 O 3 reacts with CO according to the equation Fe 2 O 3 (s) + 3CO(g) → 3CO 2 (g) + 2Fe(s) When 352 g Fe 2 O 3 reacts with excess CO, what number of moles of Fe (iron) is produced? E 400

4.41 mol Fe E 400

If g of iron react with oxygen gas to produce iron (III) oxide, how many moles of oxygen gas will be needed? E 500

1.50 moles oxygen gas E 500

In the reaction between CO and Fe 3 O 4, the theoretical yield in an experiment is calculated to be 47.2 g Fe. When a careless chemistry student carries out the experiment, the actual yield is 42.9 g Fe. Calculate the percent yield. F 100

90.9% F 100

Calculate the theoretical yield of iron in the reaction of 254 g of iron(III) oxide with 25.0 g of carbon, according to the equation 2Fe 2 O 3 (s) + 3C(s) → 4Fe(s) + 3CO 2 (g) F 200

155 g Fe F 200

When NH 3 is prepared from 28 g N 2 and excess H 2, the theoretical yield of NH 3 is 34g. When this reaction is carried out in a given experiment, only 30. g is produced. What is the percentage yield? F 300

88% F 300

If 23.4 g of MgO is produced from 59.6 g of MgCO 3, what is the percent yield? MgCO 3  MgO + CO 2 F 400

82.1 % F 400

Define percent yield F 500

Comparison of predicted and actual amounts of product F 500

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