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Abstract The purpose of this experiment was to study the rate of decomposition of methyl orange reaction at different concentration and temperature to find out its rate law rate constant and activation energy Throughout the experiment Beers Law is stating that how much light a solution absorbs is determined by the constant the distance light travels in the solution and the concentration of the absorber For every substance at every wavelength of light the extinction coefficient constant has a difference value The k exptl from slope s-1 for runs 1-6 were 00074 00086 00126 00196 00116 00116 00115 00067 and 00033 The Ea was 24 kJmolIntroduction During this experiment I was able to study the rate of the decomposition of methyl orange at different concentration and temperature In doing so I then found out other findings such as its rate law rate constant and activation energy Also in this experiment Beers law was introduced as well as the spectrophotometry which helped out the rate law analysis Methyl orange was primarily used in this experiment because it proposals a practical case of how rate and mechanism of chemical reaction are determined The color change from red to orange-yellow relates to the electrons that are distinct in the molecule when hydrogen ions are attached or detached the pH changes Commonly used in printing textiles and dyeing the compound methyl orange also known as CI Acid Orange 52 is an extremely colored compound The reason why methyl orange is red is because of the absorption of the blue-green light The purpose of the tin was to act as the reducing agent so we had to determine the concentrations when determining the rate law According to the lab manual the general rate law for the reaction would beRate-dMOdtkMOxtSn2ytH30ztTo make things less complicated we made the concentration of methyl orange much less than the tin and the hydronium ion resulting in a rate expression ofRatekSn2y0H30z0MOxtDuring the experiment we measured
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