Rate Law Lab
Lab 2: Reaction Order and Rate Laws
Khadijah Maraheel
Location: My apartment
September 27th-28th 2017
Course Number: Chem112
Abstract:
The purpose of this lab is to find the rate law of the reactants and the reactions order. My beginning thought was I would find whole numbers but that would be to easy. My answers were all with decimals. I found that my rate law Is k (HCl)1.36 (Na2S2O3)0.84. I was expecting the solution to change color but I never thought it would turn yellow/white. Majority of my previous experiments have always had darker colors as the outcome like a pink or purple. I was pretty surprised when I saw yellow/white.
Experiment:
For this experiment I determined the reaction rate, average time, moles of each solution and discovered …show more content…
What is the purpose of holding the initial concentration of one reactant constant during each trial?
The purpose is to find the product and the amount of product. If we have the initial concentration of one reactant that is constant with each trail. Then it will help us find the other reactant in the solution.
5. Rate= k [F2] [ClO2]
K((.300)/(.5M x .5M)= K(1.2m-1s-1 )
6. If the decomposition of HBr (g) into H2 (g) and Br2 (g) is known to be second order with respect to HBr. Write a balanced chemical equation for this reaction. Write the rate law for this reaction. When the concentration of HBr is 2.0 M, the rate of decomposition is 1.58x102 M/s. Calculate the value and units of the rate constant. What is the rate of this reaction when the concentration of HBr is 0.75 M?
Balance reaction: 2HBr (g) H2 (g)+ Br2 (g)
Rate law reaction: K2 (HBr)2
Rate Constant: K2(1.58 x 102) divided by (4.0M) = 3.95 x 10-3
Khadijah Maraheel
Location: My apartment
September 27th-28th 2017
Course Number: Chem112
Abstract:
The purpose of this lab is to find the rate law of the reactants and the reactions order. My beginning thought was I would find whole numbers but that would be to easy. My answers were all with decimals. I found that my rate law Is k (HCl)1.36 (Na2S2O3)0.84. I was expecting the solution to change color but I never thought it would turn yellow/white. Majority of my previous experiments have always had darker colors as the outcome like a pink or purple. I was pretty surprised when I saw yellow/white.
Experiment:
For this experiment I determined the reaction rate, average time, moles of each solution and discovered …show more content…
What is the purpose of holding the initial concentration of one reactant constant during each trial?
The purpose is to find the product and the amount of product. If we have the initial concentration of one reactant that is constant with each trail. Then it will help us find the other reactant in the solution.
5. Rate= k [F2] [ClO2]
K((.300)/(.5M x .5M)= K(1.2m-1s-1 )
6. If the decomposition of HBr (g) into H2 (g) and Br2 (g) is known to be second order with respect to HBr. Write a balanced chemical equation for this reaction. Write the rate law for this reaction. When the concentration of HBr is 2.0 M, the rate of decomposition is 1.58x102 M/s. Calculate the value and units of the rate constant. What is the rate of this reaction when the concentration of HBr is 0.75 M?
Balance reaction: 2HBr (g) H2 (g)+ Br2 (g)
Rate law reaction: K2 (HBr)2
Rate Constant: K2(1.58 x 102) divided by (4.0M) = 3.95 x 10-3