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Shalnov [3]
2 years ago
6

Given that the initial rate constant is 0.0110s−1 at an initial temperature of 21 ∘C , what would the rate constant be at a temp

erature of 150∘C for the same reaction described in Part A?
This was part A
The activation energy of a certain reaction is 45.5 kJ/mol . At 21 ∘C , the rate constant is 0.0110s−1 . I got 32.4 degree C
Chemistry
1 answer:
gulaghasi [49]2 years ago
5 0

The rate constant is mathematically given as

K2=2.67sec^{-1}

<h3>What is the Arrhenius equation?</h3>

The rate constant for a particular reaction may be calculated with the use of the Arrhenius equation. This constant can be stated in terms of two distinct temperatures, T1 and T2, as follows:

ln(\frac{K2}{K1})= (\frac{Ea}{R})*(\frac{1}{T1}-\frac{1}{T2})

Therefore

KT1= 0.0110^{-1}

T1= 21+273.15

T1= 294.15K

T2= 200  

T2=200+273.15

T2= 473.15K

Ea= 35.5 Kj/Mol

Hence, in  j/mol R Ea is

Ea=35.5*1000 j/mol R

ln(\frac{K2}{0.0110})= (\frac{35.5*1000}{8.314})*(\frac{1}{294.15}-\frac{1}{473.15}\\\\ln(\frac{K2}{0.0110})=5.492

K2/0.0110 =e^(5.492)

K2/0.0110 =242.74

K2= 242.74*0.0110

K2=2.67sec^{-1}

In conclusion, rate constant

K2=2.67sec^{-1}

Read more about rate constant

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0.120 L of hydrogen gas will be produced

Explanation:

Step 1: Data given

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Step 2: The balanced equation

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Step 3: Calculate moles Zinc

Moles Zn = mass Zn / molar mass Zn

Moles Zn = 10.0 grams / 65.38 g/mol

Moles Zn  =  0.153 moles

Step 4: Calculate moles HCl

Moles HCl = molarity * volume

Moles HCl = 0.45 M * 0.0238 L

Moles HCl = 0.01071 moles

Step 5: Calculate limiting reactant

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HCl is the limiting reactant. It will completely be consumed (0.01071 moles)

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Step 6: Calculate moles H2

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For 0.01071 moles HCl we'll have 0.005355 moles H2

Step 7: Calculate volume H2

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<em>Step 2</em>. Convert <em>miles to metres </em>

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<em>Step 3.</em> Calculate the <em>time to swim 241.4 m</em>

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