RATE OF REACTIONS. The reaction rate (rate of reaction) or speed of reaction for a reactant or product in a particular reaction is intuitively defined as how fast or slow a reaction takes place. For example‚ the oxidative rusting of iron under the atmosphere is a slow reaction that can take many years‚ but the combustion of cellulose in a fire is a reaction that takes place in fractions of a second (right). Chemical kinetics is the part of physical chemistry that studies reaction rates. The concepts
Premium Chemical kinetics Reaction rate Chemical reaction
The Effect of the Concentration of Sulphuric Acid on the Reaction Rate with Magnesium Sarah Cain SCH 4UB Mr. Lankin April 1‚ 2009 Introduction The nature of the problem is to design an investigation that examines a variable affecting the reaction rate. In this experiment‚ magnesium will be reacted with different concentrations of sulphuric acid. The reaction is shown by the following chemical equation: H2SO4 (l) + Mg (s) → MgSO4 (aq) + H2
Premium Chemical reaction Reaction rate Magnesium
reaction rates and concentration (research paper) By katie prestage what are reaction rates? The rate of reaction is the speed in which a reaction takes place. This can be measured by the rate in which a reactant is used up‚ or the rate a product is created. If a reaction has a low rate‚ it means that the particles are combining at a slow speed. If the rate is high‚ it means that the particles are coming together at a fast speed. For example‚ the rusting of iron through oxidation has a slow
Premium Reaction rate Chemical reaction Chemical kinetics
Investigating How Concentration of Acid Affects the Reaction Between Calcium Carbonate and Hydrochloric Acid Introduction ============ According to the collision theory temperature‚ concentration‚ surface area and catalysts all affect rates of reaction as shown in the diagrams below. Increasing any of these should increase the number of collisions and so increase the reaction rate up to an optimum point. Increasing the temperature causes the particles to collide with more
Premium
Any strong acid will release approximately - 57 kJ/mol of energy on neutralisation with strong base. This energy release is due to the formation of water molecules from the H+ ions from the acid reacting with the OH- ions from the base. H+(aq) + OH-(aq) H2O(l) When a weak acid is neutralised some of the energy is needed to dissociate the molecules to make the hydrogen ions available for neutralisation. The result is a value for neutralisation enthalpy lower than - 57 kJ/mol (numerically
Premium Hydrogen Acid PH
green gas. (i) Apply damp blue litmus. (Can use red litmus and just see bleaching effect.) (ii) A drop silver nitrate on the end of a glass rod into the gas. (i) litmus turns red and then is bleached white. (ii) White precipitate. (i) Non-metal‚ is acid in aqueous solution and a powerful oxidising agent (ii) It forms a small amount of chloride ion in water‚ so gives a positive result for the chloride test. Bromine Br2 (l or aq) A dark red liquid - orange-brown fumes‚ yellow-orange aqueous solution
Premium Chlorine Ammonia Sulfuric acid
Changing the Rate of Reaction PART 1: PARTICLE SIZE Question: How does changing the particle size of marble (CaCO3) affect the rate of reaction when it is added to hydrochloric acid (HCl)? Hypothesis: If I change the particle size of marble to test how to change the rate of a chemical reaction‚ than the chemical reaction with the smallest marble particles will produce CO2 the quickest because the larger the surface area‚ the more place the hydrochloric acid will have to collide with the marble
Premium Hydrochloric acid Chemical reaction Chemistry
concentrations of HSO− ‚ SO2− ‚ and H+ in a 0.20 M KHSO4 solution? (Hint: 4 4 H2 SO4 is a strong acid; Ka = 1.3 × 10−2 for HSO− .) 4 2. [15 points] Calculate the pH of 1.00 L of the buffer 1.00 M CH3 COONa/1.00 M CH3 COOH (pKa = 4.74) before and after the addition of (a) 0.080 moles NaOH and (b) 0.12 moles HCl. (Assume there is no change in volume). 3. [10 points] The following reaction is found to be first order in A: A −→ B + C If half of the starting quantity of A is used up after
Premium Acid dissociation constant Enzyme inhibitor Chemical kinetics
percentage errors. OBJECTIVE The objective of this experiment is to determine the order with respect to permanganate ion and to oxalic acid concentration for the reaction of potassium permanganate and oxalic acid solutions. Other goals include‚ writing a rate equation and determining the effect of increased temperature on the rate of this reaction. MATERIALS AND EQUIPMENT The materials required for this experiment include the following: • 2-50ml Burets • 60 mL of 0.755M H2C2O4 • 60
Premium Potassium permanganate Laboratory glassware Carboxylic acid
The effect of temperature on a reaction rate In this experiment I shall be investigating how temperature affects the rate of reaction Rates of reaction The Factors that affect the rate of reaction are temperature‚ surface area‚ concentration‚ catalysts‚ light and pressure Surface area – Surface area is the amount of solid surface that is available for reaction - Only affects solids so this will not affect our
Premium Chemical reaction Chemistry Reaction rate