Answer:
ΔH=15000
J = 15KJ
Explanation:
In this exercise you have find the enthalpy of reaction this is the difference between enthalpy of reactans and products,
For the following equation
H2A(aq) + 2 BOH(aq) → B2A(aq) + 2 H2O(l)
We know that 0.20 moles of BOH reacted with excess amount of H2A solution and 1500. J
so,
(2mol/0,2mol)*1500J=15000J
for de reactions exothermics tha enthalpy is negative so:
ΔH=15000
J = 15KJ
The molar extinction coefficient is 15,200 .
The formula to be used to calculate molar extinction coefficient is -
A = ξcl, where A represents absorption, ξ refers molar extinction coefficient, c refers to concentration and l represents length.
The given values are in required units, hence, there is no need to convert them. Directly keeping the values in formula to find the value of molar extinction coefficient.
Rewriting the formula as per molar extinction coefficient -
ξ =
ξ =
Performing multiplication in denominator to find the value of molar extinction coefficient
ξ =
Performing division to find the value of molar extinction coefficient
ξ = 15,200
Hence, the molar extinction coefficient is 15,200 .
Learn more about molar extinction coefficient -
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C or A. I can’t decide tho. I know most def it’s gotta be one of them two.
<u>Answer:</u> The mass of needed is 0.96 grams
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
.....(1)
- <u>For </u><u> :</u>
Given mass of = 320.0 mg = 0.320 g (Conversion factor: 1 g = 1000 mg)
Molar mass of = 20 g/mol
Putting values in equation 1, we get:
For the given chemical equation:
By Stoichiometry of the reaction:
1 mole of is produced from 3 moles of
So, 0.016 moles of will be produced from = of
Now, calculating the mass of from equation 1, we get:
Molar mass of = 20 g/mol
Moles of = 0.048 moles
Putting values in equation 1, we get:
Hence, the mass of needed is 0.96 grams