Answer:
710,33 g NO2
Explanation:
2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
(800 g octane) / (114.2293 g C8H18/mol x (25/2)) = 87.54 mol O2 used to combust the octane
= 15.44 mol O2 used to form NO2
O2 + 2NO → 2NO2
(15.44 mol O2) x (2/2) x (46.0056 g NO2/mol) = 710,33 g NO2
Answer: The molecular formula for the given compound is
Explanation : Given,
Percentage of C = 85.7 %
Percentage of H = 14.3 %
Let the mass of compound be 100 g. So, percentages given are taken as mass.
Mass of C = 85.7 g
Mass of H = 14.3 g
To formulate the empirical formula, we need to follow some steps:
Step 1: Converting the given masses into moles.
Moles of Carbon =
Moles of Hydrogen =
Step 2: Calculating the mole ratio of the given elements.
For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 7.14 moles.
For Carbon =
For Hydrogen =
Step 3: Taking the mole ratio as their subscripts.
The ratio of C : H = 1 : 2
The empirical formula for the given compound is
Mass of empirical formula = = 1(12) + 2(1) = 14 g/eq.
Now we have to determine the molar mass of compound.
As, 112 mL of volume contains 0.21 g of compound
So, 22400 mL of volume contains of compound
For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.
The equation used to calculate the valency is :
We are given:
Mass of molecular formula = 42 g/mol
Mass of empirical formula = 14 g/mol
Putting values in above equation, we get:
Multiplying this valency by the subscript of every element of empirical formula, we get:
Thus, the molecular formula for the given compound is
Answer:
Explanation:
The pressure is constant, so, to calculate the volume, we can use Charles' Law:
\dfrac{V_{1}}{T_{1}} = \dfrac{V_{2}}{T_{2}}
Data:
V₁ = ?; T₁ = 450 K
V₂ = 103.4 L; T₂ = 284.9 K
Calculation:
