Introduction: Reaction of a compound with water can result in a splitting, or lysis, of the compound into two parts. Organic molecules containing a group of atoms called an ester can be hydrolyzed by water to form a –COOH group (carboxylic acid) and an HO-- group (alcohol) as follows: RCOOR’ + H2O ( RCOOH + HOR’ This reaction is spontaneous for almost all esters but can be very slow under typical conditions of temperature and pressure. The reaction occurs at a much faster rate if there is a significant
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Determination of the Reaction Rate of Mg and HCl Alex Skartvedt Alex Skartvedt, Melanie Ho, Christina Olson, Thor Swerdykiak November 11, 2015 Fall 2015 Semester Abstract: The experimental rate law of the reaction: 2HCl(aq)+Mg(s)→MgCl2(aq)+H2(g) is being determined because kinetics play a large role in the reactions happening in everyday life. The rate law, k value will be obtained in the experiment. To obtain the information a pressure probe was connected to an Erlenmeyer flask in
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BMW 6HP19 – 6HP21 Transmission fluid level procedures A) Transmissions fluid level checking. 1) The transmission fluid temperature must be between 30°C and 35°C before checking can begin. Use test equipment to determine the trans temperature. 2) The vehicle must be level with engine running at idle speed and air conditioning turned on. 3) Step on the brakes firmly, apply parking brake fully and shift to D and R, briefly pausing in each position before shifting back to the Park position.
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The rate of a chemical reaction can be raised by temperature, concentration of solutions, catalysts, etc. Increasing the surface area of a solid reactant is one way the rate of reaction can be sped up. If the surface area is increased, then more particles are exposed to reactants, there are more collisions, and these two variables overall speed up the rate of reaction. (BBC, 2014) A solid that is found in a solution can only react when particles collide with the surface area of the solid. When the
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2 ASSIGNMENT 1 Question 1 (a) Rate of formation = 13d[O2]dt Rate of disappearance = - 12d[O3]dt (b) Rate of formation = 12d[HF]dt = d[O2]dt Rate of disappearance = - 12d[HOF]dt (c) Rate of formation = 12d[BrNO]dt Rate of disappearance = - 12d[NO]dt= - d[Br2]dt Question 2 2NO(g) + H2(g) N2O(g) + H2O(g) (a) Rate = k[NO]2[H2] (b) 0.005 = k(0.075)2(0.400) 0.005 = k(2.25 x 10-3) k = 2.22 M-2 s-1 Question 3 Temperature (K) | Rate constant (M/s) | 1/T (K-1) | ln k |
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Investigating Rates of Reaction between Hydrochloric Acid and Magnesium Introduction What is Rate of Reaction? The reaction rate or rate of reaction for a reactant or product in a particular reaction is intuitively defined as how fast a reaction takes place. For example, the oxidation of iron under the atmosphere is a slow reaction which can take many years, but the combustion of butane in a fire is a reaction that takes place in fractions of a second. In this case how fast Magnesium reacts
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experiment, the rate law and rate constant for a reaction of oxalic acid with permanganate were determined. Every chemical reaction ranges from hours to femtoseconds to occur. The rate of a chemical reaction can be determined by assessing the change in either the reactant or product in a given time or point (Connors, 1990). It is important to take account of the stoichiometric ratios of each component, regardless as to which compound is chosen to determine the rate. The study of the rates of chemical
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Introduction Enzymes are biological catalysts. Catalysts are substances that increase the rate of chemical reactions without being used up themselves. Enzymes are also proteins. They all have different and complex shapes that allow smaller molecules to fit into them. The place where these substrate molecules fit is called the active site. The shape of an enzyme can change; its active site may no longer work. It is said the enzyme is denatured. They can be denatured by high temperatures or extremes
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Ni (s)? 2. 3Ca (s) + 2Al(NO3)3 (aq) 3Ca(NO3)2 (aq) + 2Al (s) a) Predict the voltage for an electrochemical cell based on the above reaction. Assume standard conditions. 3. Use the Eo values to determine if the following reaction is spontaneous or not: Mg2+ (aq) + Cu (s) Mg (s) + Cu2+ (aq) 4. balance the following reaction b) Zn (s) + NO3- (aq) Zn2+ (aq) + NH4+ (aq) (acidic) c) Cl2 (aq) Cl- (aq) + ClO3- (aq) (basic) d) MnO4-(aq) + Sn2+ (aq)
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Michaelis-Menten Kinetics: The Enzyme-Catalyzed Hydrolysis of Sucrose1 Background Of the numerous chemical reactions whose kinetics have been studied, some of the most interesting and complex are those which take place in living organisms. These reactions, when studied under non-biological conditions (lack of organisms and their various biomolecules), are often exceptionally slow: often hours or days, and sometimes even years are required before equilibrium is reached. Yet life requires seconds
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