pls help me with the questions d11/13/1 Revised 11/13/17 Data Analysis 1. Was th

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pls help me with the questions

d11/13/1 Revised 11/13/17 Data Analysis 1. Was the reaction zero, first, or second order, with respect to the concentration of crystal violet (use room temperature data)? Explain 2. Calculate the rate constants, k, at both your linear curve. Include the correct units for the rate constant. Note. This constant is sometimes referred to as the pseudo rate constant, because it does not take into account the effect of the other reactant, OH temperatures, using the slope of the Curve Fit for 3. Write the correct rate law expression for the reaction, in terms of crystal violet (omit OH) At 4. Use your value of k to determine the half-life of the reaction at room temperature. s. Use the two-point version of the Arrhenius equation Ini-E(11 Ink (7,-7/, where R-8314 J/cK.mol), to determine the activation energy, Ea, for this reaction with respect to crystal violet (use room temperature and ice bath data) Page 3 of 3

Explanation / Answer

1. From the plots

the order with respect to crystal violet is 1, first-order reaction.

2. rate constant (k2)

at T2 = 25.3 oC + 273 = 298.3 K

k2 = -[ln(0.469) - ln(0.556)]/30 = 0.0057 s-1

rate constant (k1)

at T1 = 2.7 oC + 273 = 295.7 K

k1 = -[ln(0.814) - ln(0.846)]/30 = 0.0013 s-1

3. rate law,

rate = k[CV]

4. half-life (t1/2) = ln(2)/k

average k from two parts = 0.0035 s-1

t1/2 = ln(2)/0.0035 = 198.04 s

5. Arrhenius equation,

ln(k2/k1) = Ea/R[1/T1 - 1/T2]

with,

R = gas constant

Ea = activation energy

feeding values from 2.,

ln(0.0057/0.0013) = Ea/8.314[1/275.7 - 1/298.3]

Ea = 44.720 kJ/mol

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