Answer:
The mole fraction of nitrogen is 0.52
Explanation:
Provided information:
Temperature = 31.2 °C
Pressure = 870.2 mmHg
Volume = 15.1 L
Mass of the mixture = 24.1 g
Mole fraction of nitrogen =?
Process:
Converting pressure:
870.2 / 760 = 1.12 atm
Converting temperature:
31.2 + 273 = 304.2 K
Total moles calculation:
PV = nRT
n = PV/RT
n = 1.12 atm × 15.1 L / 0.0821 L.atm. mol⁻¹.K⁻¹ × 304.2 K
n = 16.9 L.atm. / 25 L.atm. mol⁻¹
n = 0.676 mol
Let x be the number of moles of nitrogen.
Thus, the moles of CO₂ = 0.676 - x
The mass of nitrogen = x mol × 28 g/mol, and for CO₂ the mass = 44 g/mol (0.676 - x)
We have 24.1 = 28x + (29.7 - 44x)
Rearranging gives: 24.1 - 29.7 = 28x - 44x
-5.6 = -16 x
Therefore, x = 0.35
Mole fraction of nitrogen:
Mole fraction of nitrogen = moles of nitrogen / total moles
Mole fraction of nitrogen = 0.35 mol / 0.676 mol
Mole fraction of nitrogen = 0.52
Response:
Clarification:
Hello,
In this scenario, since a single drop equates to 0.05 mL of the solution provided, with a concentration of 0.02 g/mL, the mass of oleic acid in one drop calculates to:
Best wishes.
Answer:- 0.134 seconds
Solution:- The speed is given as 
and the circumference is 24900 miles which is same as the distance light have to covered. It asks to calculate the time required to cover this distance by the light.
Unit conversion is needed from miles to meters since the speed is given in meters per second.
1 mile = 1609.34 meters
Thus, 
= 40072566 meters
Now, 
Rearranged for time, that gives: 
Inserting the values:
= 0.134 seconds
Hence, light would take 0.134 seconds to traverse the indicated distance. The answer without the unit is 0.134.
In a 100 g sample of the compound, there are 63.57 g of carbon, 6 g of hydrogen, 9.267 g of nitrogen, and 21.17 g of oxygen. First, convert these masses into moles (n) using the formula n = m/M, where M is the molar mass from the periodic table.
For carbon: 63.57 g C -> 63.57 g C / 12.01 g/mol = 5.29 moles C.
For hydrogen: 6 g H -> 6 g H / 1.008 g/mol = 5.95 moles H.
For nitrogen: 9.267 g N -> 9.267 g N / 14.01 g/mol = 0.6615 moles N.
For oxygen: 21.17 g O -> 21.17 g O / 16.00 g/mol = 1.32 moles O.
Thus, the mole ratio looks like this: C 5.29 H 5.95 N 0.6615 O 1.32.
Now, divide each value by the smallest number (1.32): C 4 H 4.5 N 0.5 O 1.
To eliminate fractions, multiply all values by 2, yielding C8H9N1O2.
Now, all numbers are integers! Hence, the empirical formula is C8H9NO2.
Although the empirical formula isn't always the same as the molecular formula, in this instance, it corresponds to acetaminophen.
