For the following, convert the word equation to a formula equation, BUT DO NOT BALANCE
1 answer:
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Answer : The mass of hydrogen gas consumed will be, 4.5 grams
Explanation : Given,
Mass of = 21 g
Mass of = 18 g
Molar mass of = 28 g/mole
Molar mass of = 2 g/mole
First we have to calculate the moles of and
.
Now we have to calculate the limiting and excess reagent.
The balanced chemical reaction is,
From the given balanced reaction, we conclude that
As, 1 mole of react with 3 moles of
So, 0.75 moles of react with
moles of
From this we conclude that, is an excess reagent because the given moles are greater than the required moles and
is a limiting reagent because it limits the formation of product.
The moles of hydrogen gas consumed = 2.25 mole
Now we have to calculate the mass of hydrogen gas consumed.
Therefore, the mass of hydrogen gas consumed will be, 4.5 grams
Answer:
1) Eₐ = 100.3 kJ/mol
2) k = 7.62×10⁻⁴ M⁻¹s⁻¹
Explanation:
1) Make an Arrhenius graph by plotting ln(k) on the y-axis and 1/T on the x-axis (don't forget to convert temperature to Kelvin).
The slope of the line is equal to -Eₐ/R.
-Eₐ/R = -12065
Eₐ = 100,300 J/mol
Eₐ = 100.3 kJ/mol
2) Since we know the slope of ln(k) vs 1/T is -Eₐ/R, we can say:
-Eₐ/R = (ln(k₂) − ln(k₁)) / (1/T₂ − 1/T₁)
Plug in values and solve for k:
-(108,000 J/mol) / (8.314 J/mol/K) = [ln(k) − ln(1.0×10⁻³)] / [1/(35+273.15 K) − 1/(37+273.15 K)]
-12990 = [ln(k) + 6.91] / (2.09×10⁻⁵ K⁻¹)
-0.272 = ln(k) + 6.91
ln(k) = -7.18
k = 7.62×10⁻⁴ M⁻¹s⁻¹
