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Chemistry 11 Stoichiometry Review Assignment
Name: ______________________________ Date: ______________ Block: _____
Answer the following practice questions on a separate page
Define the following terms:
- Stoichiometry: quantitative relationships among substances as they participate in chemical reactions
- Stoichiometric ratio: the molar ratio of substances in a chemical reaction (coefficients in a balanced chemical equation)
- Limiting reactant the reactant in a chemical reaction is the substance that is totally consumed when the chemical reaction is complete. The amount of product formed is limited by this reagent , since the reaction cannot continue without it.
- Excess reactant In a chemical reaction, reactants that are not use up when the reaction is finished are called excess reagents.
- Percent yield is calculated to be the experimental yield divided by theoretical yield multiplied by 100%.
(Mole-Mole Conversions)
- The combustion of the organic fuel, decane, is outlined in the chemical equation below. You must balance the equation in order to answer the subsequent questions a-c. __2__C 10 H 22 + _31_O 2 __20__CO 2 + __22__H 2 O a. How many moles of CO 2 are produced if 5.0 moles of C 10 H 22 react with an excess of O 2? b. How many moles of O 2 react with 0.75 moles of C 10 H 22? c. How many moles of O 2 would be required to produce 4.0 moles of H 2 O?
- Use the following equation to solve the problems below:
3 SiO 2 + 4 Al 3 Si + 2 Al 2 O 3 a. If 6.0 moles of SiO 2 react, how many moles of: i. Al react? ii. Si are produced? iii. Al 2 O 3 are produced?
b. If 2.5 moles of Al 2 O 3 are produced, how many moles of: i. Al react? ii. SiO 2 react?
(Mole-Mass / Mass-Mole Conversions)
- N 2 + 2O 2 → N 2 O 4
a) If 15.0g of N 2 O 4 was produced, how many moles of O 2 were required?
15.0g N 2 O 4 1 mol N 2 O 4 2 mol O 2 92.0g N 2 O 4 1 mol N 2 O 4
= 0.326 mol O (^2)
b) If 4.0x10-3^ moles of oxygen reacted, how many grams of N 2 were needed?
4.0x10-^3 mol O 2 1 mol N 2 28.0g N 2 2 mol O 2 1 mol N 2
= 5.6x10 -2^ g N (^2)
- Cu + 2AgNO 3 → Cu(NO 3 ) 2 + 2Ag How many moles of Cu are needed to react with 3.50g of AgNO 3?
3.50g AgNO 3 1 mol AgNO 3 1 mol Cu 169.9g AgNO 3 2 mol AgNO 3
= 1.03x10 -2^ mol Cu
- Cu + 2AgNO 3 → 2Ag + Cu(NO 3 ) (^2) How many grams of silver are produced when 36.92g of copper react?
36.92g Cu 1 mol Cu 2 mol Ag 107.9g Ag 63.5g Cu 1 mol Cu 1 mol Ag
= 125g Ag
- ___Al 2 (SO 4 ) 3 + ___Ca(OH) 2 →___Al(OH) 3 + ___CaSO 4 Balance and answer the following questions. Al 2 (SO 4 ) 3 + 3Ca(OH) 2 → 2 Al(OH) 3 + 3CaSO (^4) a. What mass of aluminum (III) hydroxide are produced if 165.7g of aluminum (III) sulfate react?
165.7g Al 2 (SO 4 ) 3 1 mol Al 2 (SO 4 ) 3 2 mol Al(OH) 3 78.0g Al(OH) 3 342.3g Al 2 (SO 4 ) 3 1 mol Al 2 (SO 4 ) 3
= 75.5g Al(OH) 3
b. How many grams of calcium hydroxide are needed to form 6.35g of calcium sulphate?
6.35g CaSO 4 1 mol CaSO 4 3 mol Ca(OH) 2 74.1g Ca(OH) (^2) 136.2g CaSO 4 3 mol CaSO 4 1 mol Ca(OH) (^2)
= 3.45g Ca(OH) 2
(Mass- Volume/ Volume-Volume Conversions)
- Given the following equation: 3 NO 2 (g) + H 2 O(l) 2 HNO 3 (aq) + NO(g) Assume STP
a. What mass of water is required to react with 15.5 L of Nitrogen dioxide? b. What volume of Nitrogen monoxide would be produced from 100.0 g of water? c. If 42.0 L of NO (g) is produced, what volume of NO 2 (g) reacted?
- When Magnesium reacts with Nitric Acid, Hydrogen gas and aqueous Magnesium nitrate are formed. What volume of Hydrogen gas will be produced if 40.0 g of Magnesium is reacted with an excess of Nitric Acid?
- The corrosion (rusting) of iron is represented as follows: (at STP)
3 O2 (g) + 4 Fe (^) (s) 2 Fe 2 O3 (s)
a. What volume of Oxygen gas would be required to produce 16.0 g of Fe 2 O 3? b. What mass of Iron would be required to react with 10.0 L of O 2 gas?
- Mercury (II) oxide decomposes when heated to produce liquid Mercury and Oxygen gas. What mass of Mercury (II) oxide would be required to produce 30.5 L of Oxygen gas? (Assume STP)
- How many mL of 2.00M HNO3 is needed to consume 5.4g of aluminum?
2Al + 6HNO 3 2Al(HNO 3 ) 3 + 3H 2 5.4g Al 1mol Al 6 mol HNO 3 27.0g Al 2 mol Al = 0.60 molsHNO 3
[HNO 3 ] = # mols ÷ volume So, Volume = mols ÷ [HNO 3 ] =0.60mol ÷2M = 0.3 L (x 1000)= 3.0 x10 2 mL HNO (^3)
You calculate that using a certain amount of beryllium and hydrochloric acid you can produce 10.7g of beryllium chloride. You perform the experiment and only collect 4.5g What is the percent yield for the reaction? 42% yield
- Determine the percent yield for the reaction between 44.5g of zinc sulphide and 13.3g of oxygen, if 18.4g of zinc oxide is recovered with an unknown amount of Sulphur dioxide. 81.6% yield
- A reaction was carried out according to the following equation:
FeBr 2 + 2 KCl FeCl 2 + 2 KBr a) What is the theoretical yield of iron (II) chloride if 34.00 grams of iron (II) bromide was used in the reaction with excess potassium chloride? 20.00g FeCl (^2) b) What is the percent yield of iron (II) chloride if the actual yield is 4.00 grams? 20.0% yield
- 17.5g of C(s) are reacted with 39.5g of SO2(g) according to the equation:
5C(s) + 2SO2(g) CS2(s) + 4CO2(g)
- What mass of CS2(s) is produced? 22.2g CS 2
- What mass of the excess reactant will be left over? 2.1g SO 2 left over
