Everything Science Grade 12

CHAPTER 3. REACTION RATES 3.4 Changes in mass: The rate of a reaction that produces a gas can alsobe measured by calculating th ...

3.5 CHAPTER 3. REACTION RATES Beaker Solution A (cm^3 ) Water (cm^3 ) Solution B (cm^3 ) Time (s) 1 60 20 10 2 50 30 10 3 40 40 ...

CHAPTER 3. REACTION RATES 3.5 Even at a fixed temperature, the energy of the particles varies, meaning that only some of them wi ...

3.5 CHAPTER 3. REACTION RATES DEFINITION: Catalyst A catalyst speeds up a chemical reaction, without being altered in any way. I ...

CHAPTER 3. REACTION RATES 3.5 Now add the copperpieces to the same testtube. What happens tothe rate at which the gas is produc ...

3.6 CHAPTER 3. REACTION RATES (a) Write a balanced chemical equation for thisreaction. (b) The rate of the reaction is determine ...

CHAPTER 3. REACTION RATES 3.6 Observations: You should notice that inthe beaker that is uncovered, the water level drops quickly ...

3.6 CHAPTER 3. REACTION RATES Open and closed systems ESCAW An open system is one in which matteror energy can flow intoor out o ...

CHAPTER 3. REACTION RATES 3.6 DEFINITION: A reversible reaction A reversible reaction isa chemical reaction that can proceed in ...

3.6 CHAPTER 3. REACTION RATES calcium carbonate & hydrochloric acid limewater delivery tube rubber stopper rubber stopper Di ...

CHAPTER 3. REACTION RATES 3.6 forward reaction is highand the rate of the reverse reaction is low. Asthe reaction proceeds, the ...

3.7 CHAPTER 3. REACTION RATES 3.7 The equilibrium constant DEFINITION: Equilibrium constant The equilibrium constant (Kc), relat ...

CHAPTER 3. REACTION RATES 3.7 k 1 k 2 = [C][D] [A][B] or, if the constants k 1 and k 2 are simplified to a singleconstant, the e ...

3.7 CHAPTER 3. REACTION RATES The meaning of Kcvalues ESCBB The formula for Kchas the concentration of the products in the numer ...

CHAPTER 3. REACTION RATES 3.7 Calculate the value of Kc. SOLUTION Step 1 : Write the equation forkc Kc= [NO][SO 3 ] [SO 2 ][NO 2 ...

3.7 CHAPTER 3. REACTION RATES [O 2 ] = 3 mol· dm−^3 6 = 0. 5 mol· dm−^3 Example 4: Equilibrium calculations QUESTION Initially 1 ...

CHAPTER 3. REACTION RATES 3.7 NH 3 N 2 H 2 Start of reaction 1.4 0 0 Used up 0.8 0 0 Produced 0 0.4 1.2 Equilibrium 0.6 0.4 1.2 ...

3.7 CHAPTER 3. REACTION RATES H 2 (g) I 2 2HI Start of reaction 0.496 0.181 0 Used up 0.1735 0.1735 0 Produced 0 0 0.347 Equilib ...

CHAPTER 3. REACTION RATES 3.8 3.8 Le Chatelier’s principle ESCBC A number of factors caninfluence the equilibriumof a reaction. ...

3.8 CHAPTER 3. REACTION RATES The same would be true if the concentration ofthe product (NH 3 ) was changed. If [NH 3 ] decreas ...