Chapter 4
... KHC8H4O4) is used as the titrant. KHP has one acidic hydrogen. 41.20 mL of the KHP solution is used to titrate the sodium hydroxide solution to the endpoint. What is the resulting concentration of the ...
... KHC8H4O4) is used as the titrant. KHP has one acidic hydrogen. 41.20 mL of the KHP solution is used to titrate the sodium hydroxide solution to the endpoint. What is the resulting concentration of the ...
Thermochem problems
... We can use tabulated ΔH values to calculate the enthalpy of reactions ΔH depends on amounts of reactants and products and their initial and final states ΔH is a state function, so does not depend upon how we get from reactants to products Example: N2(g) + 3H2(g) 2 NH3(g) Hrxn = ? N2(g) + 3H2(g) ...
... We can use tabulated ΔH values to calculate the enthalpy of reactions ΔH depends on amounts of reactants and products and their initial and final states ΔH is a state function, so does not depend upon how we get from reactants to products Example: N2(g) + 3H2(g) 2 NH3(g) Hrxn = ? N2(g) + 3H2(g) ...
5.7 Quantity Relationships in Chemical Reactions
... You start with 20 kernels of popping corn, but you end up with only 16 pieces of popcorn. In other words, not all the kernels “popped”. • What is the theoretical number of popcorn that we could expect? • What is the actual percent of the kernels popped? Note that in all the examples of chemical reac ...
... You start with 20 kernels of popping corn, but you end up with only 16 pieces of popcorn. In other words, not all the kernels “popped”. • What is the theoretical number of popcorn that we could expect? • What is the actual percent of the kernels popped? Note that in all the examples of chemical reac ...
Quiz Samples
... Gas occupies all the volume available T F Calculate the final pressure formed after the containers 1 and 2 were connected: Total volume= 1L+2L=3L; total amount of gas Container 1, 1L under 2 atm of gas Container 2, 2L under 1 atm of gas at normal pressure= 4L*atm (2 L in Container 1 and 2 L in Conta ...
... Gas occupies all the volume available T F Calculate the final pressure formed after the containers 1 and 2 were connected: Total volume= 1L+2L=3L; total amount of gas Container 1, 1L under 2 atm of gas Container 2, 2L under 1 atm of gas at normal pressure= 4L*atm (2 L in Container 1 and 2 L in Conta ...
Chemistry COS 2011-2012
... Reaction rates and equilibrium can be controlled by changing concentration, pressure and temperature of the reactants and products. Catalysts speed up reactions by providing an alternative pathway with a lower activation energy. When a reaction is at equilibrium, the rates do not change. Le Chatelie ...
... Reaction rates and equilibrium can be controlled by changing concentration, pressure and temperature of the reactants and products. Catalysts speed up reactions by providing an alternative pathway with a lower activation energy. When a reaction is at equilibrium, the rates do not change. Le Chatelie ...
Learning objectives - The John Warner School
... surface area affects the rate. Encourage students to consider what the variables are in the experiment [time, temperature, concentration and volume of acid, mass of marble]. Students should then decide on the appropriate values of each and detail which variables should be control variables. The inve ...
... surface area affects the rate. Encourage students to consider what the variables are in the experiment [time, temperature, concentration and volume of acid, mass of marble]. Students should then decide on the appropriate values of each and detail which variables should be control variables. The inve ...
HOCl wt/wt 0.06 x mL 90 one cy
... change, any precipitate (why?), is it a homogeneous mixture, bubbling of gas? Was there any odour? What was the appearance of the product after recrystallization. Can you explain why these changes are occurring? Compare actual melting point to literature. Is it pretty accurate or any discrepancies? ...
... change, any precipitate (why?), is it a homogeneous mixture, bubbling of gas? Was there any odour? What was the appearance of the product after recrystallization. Can you explain why these changes are occurring? Compare actual melting point to literature. Is it pretty accurate or any discrepancies? ...
Chapter 9 Stoichiometry
... If everything in the reaction went according to plan, and all of the reactant(s) reacted, this is how much product should be made. This is NOT the same as the actual yield- amount that is produced based on an experiment Error occurs, so actual yield is less than the ...
... If everything in the reaction went according to plan, and all of the reactant(s) reacted, this is how much product should be made. This is NOT the same as the actual yield- amount that is produced based on an experiment Error occurs, so actual yield is less than the ...
N Goalby chemrevise.org 1 2.5 Transition Metals Substitution
... Catalysis Catalysts increase reaction rates without getting used up. They do this by providing an alternative route with a lower activation energy. Transition metals and their compounds can act as heterogeneous and homogeneous catalysts. ...
... Catalysis Catalysts increase reaction rates without getting used up. They do this by providing an alternative route with a lower activation energy. Transition metals and their compounds can act as heterogeneous and homogeneous catalysts. ...
Part II - American Chemical Society
... c. XeF2 is nonpolar. Both Xe–F bond dipoles are the same size, but due to the linear geometry they offset each other. XeF4 is nonpolar. All Xe–F bond dipoles are the same size, but due to the square planar geometry they offset each other. XeO3 is polar. The Xe–O bond dipoles are the same size, and t ...
... c. XeF2 is nonpolar. Both Xe–F bond dipoles are the same size, but due to the linear geometry they offset each other. XeF4 is nonpolar. All Xe–F bond dipoles are the same size, but due to the square planar geometry they offset each other. XeO3 is polar. The Xe–O bond dipoles are the same size, and t ...
Chemical Equations
... Thus, the same collection of atoms is present after a reaction as before the reaction. The changes that occur during a reaction just involve the rearrangement of atoms. A chemical equation shows how the atoms are rearranged. ...
... Thus, the same collection of atoms is present after a reaction as before the reaction. The changes that occur during a reaction just involve the rearrangement of atoms. A chemical equation shows how the atoms are rearranged. ...
2010 Chemistry Written examination 2
... One way to remove these nitrogen oxides is to treat the chimney gases with ammonia. This treatment converts the oxides of nitrogen in the chimney gases to nitrogen and water. These are then released into the atmosphere. a. i. Determine the coefficients that correctly balance the equation for this re ...
... One way to remove these nitrogen oxides is to treat the chimney gases with ammonia. This treatment converts the oxides of nitrogen in the chimney gases to nitrogen and water. These are then released into the atmosphere. a. i. Determine the coefficients that correctly balance the equation for this re ...
Chemistry Exam 2 Specifications and Sample Exam
... B. a colourless gas at the cathode and a metallic coating on the anode. C. a coloured liquid at the anode and a metallic coating on the cathode. D. a colourless gas at the anode and a coloured liquid at the cathode. Question 11 Information supplied on the electrochemical series about Fe2+(aq) indica ...
... B. a colourless gas at the cathode and a metallic coating on the anode. C. a coloured liquid at the anode and a metallic coating on the cathode. D. a colourless gas at the anode and a coloured liquid at the cathode. Question 11 Information supplied on the electrochemical series about Fe2+(aq) indica ...
Catalysis
Catalysis is the increase in the rate of a chemical reaction due to the participation of an additional substance called a catalyst. With a catalyst, reactions occur faster and require less activation energy. Because catalysts are not consumed in the catalyzed reaction, they can continue to catalyze the reaction of further quantities of reactant. Often only tiny amounts are required.