Answer:
3.47 × 10¹ M⁻¹ h⁻¹
Explanation:
From the question, it's clearly depicted that it is a second order reaction rate.
NOW, rate constant for second order reaction can be given as:
k(t)=
Given that:
t = 24 hours
Let the initial concentration of reactant
Final concentration
∴
k(t)=
k(24)hours = 833.33 M⁻¹
k =
k = 34.72 M⁻¹ h⁻¹
k = 3.472 × 10¹ M⁻¹ h⁻¹
∴ the value of the rate constant (k) = 3.472 × 10¹ M⁻¹ h⁻¹
The answer is -0.22 for the total impact of velocity 1.1 seconds -5.0=-
Units of measurement should be shown on the x axis.
Answer:
92.01 g/mol
Explanation:
So first you need to find the empirical formula by the percents. That would be, assuming that you have 100 grams of the the sample, divide each quantity of each element found by its respective molar mass.
30.4 g of N ÷ 14 g/mol N= 2.17 mol of N
69.6 g of O ÷ 16g/mol= 4.35 mol of O
You can establish now the empirical formula.
N2.17O4.35,
but since you can't have a decimal subscript, you divide each subscript by the minimum subscript
NO2
So then you're said that the molecular formula derived from that empirical formula has 2 nitrogen, so you multiply all the subscripts, by 2:
N2O4
-Dinitrogen Tetraoxide
-Nitrogen oxide (IV)
Then all you have to do is find the molecular mass of the compound using the periodic table and what you obtain is the molar mass.
remember: molecular mass is correspondent to molar mass.