• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

The Rate of Reaction of Metals With Acid

Extracts from this document...

Introduction

The Rate of Reaction of Metals With Acid Introduction Chemical reactions are, to a certain extent, reversible. The rate of reaction can help of to find out the forward reaction to continue for some time enough products. The concentration of the reactant depends on the difference in the rate of the forward and reverse reactions. Carrying out experiment can found the rate of equation, which is affected by concentration. A graph can show how concentration alters depending on the value of the rate constant, k. It should be plot concentration against time. A graph can be show for the increase in concentration of a product during a typical reaction. ...read more.

Middle

Magnesium chloride and hydrogen gas are formed. The temperature of both mixtures is the same. The higher concentration of acid has the effect of increasing the number of collisions between particles that can react with each other. So, the number of collisions that reach the activation energy also increases. The initial rate of the reaction is much faster in many reactions where concentration reagents are used. A graph can plot by the Arrhenius equation: ln k = constant - EA (1/T) / R where k is the rate constant of the reaction. R is the gas constant, 8.31 J K-1 mol-1 and T is the temperature in kelvins. ...read more.

Conclusion

Implementing Goggles should be wear all the time when doing experiments. A white gas is produced by the experiment, which is poisonous for the health. The results are repeated and take the mean value. Surrounding temperature should not be having a big difference when each experiment carries out. HCl (1M)/cm3 Mg/(g) Initial Temperature/? Final Temperature/? Run 1 4 0.503 20 34 Run 2 6 0.503 19 43 Run 3 16 0.503 20 58 Concluding and evaluating When the volume of hydrochloride acid increases, the temperature rise up quickly whiles the magnesium powder keep constant. The differences between the initial temperature and the final temperature are also big. This means that Mg react with acid vigorously. Temperature might not be read accurately because it is hard to read the highest temperature. It might be drop slightly since the surrounding temperature lower than the reaction temperature. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Patterns of Behaviour section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related GCSE Patterns of Behaviour essays

  1. Determine the rate equation for the reaction of hydrochloric acid with magnesium metal, and ...

    = ln(collision rate) - EA/R � (1/T) where k is the rate constant of the reaction, R is the gas constant 8.31 J K-1 mol-1, EA is the activation energy of the reaction in J mol-1, and T is the temperature in Kelvin.

  2. The aim of the investigation is to examine the kinetics involved in the reactions ...

    Temperature also influences the rate at which the reaction occurs. Ref: Chemistry in Context, G.C. Hill & J.S. Holman, p411. A graph to show the activation energy of a reaction: Ref: Chemistry for Advanced Level, Peter Cane, p158. The reaction profile above shows that the reactants are higher in terms of energy than the products.

  1. Find out how the rate of hydrolysis of an organic halogen compound depends on ...

    plastic gloves Once again, the equipment chosen in this experiment were such that accuracy, precision and reliability are ensured. For example, a volumetric flask was used because of its high degree of accuracy in quantitative analysis. It has an error of 0.2 cm3, as quoted by British Standards.

  2. The rate of reaction of metals with acid.

    A first-order reaction has a constant half-life. The following graph is a graph to show zero order The concentration falls at a steady rate with time. Half-life decreases with time which indicates 0 order The following graph below shows a graph of first order The concentration halves in equal time intervals, which therefore means that it has a constant half-life.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work