Answer:
N₂O₅
Explanation:
From the question given above, the following data were obtained:
Mass of compound = 7.546 g
Mass of nitrogen (N) = 1.957 g
Empirical formula =?
Next, we shall determine the mass of oxygen present in the compound. This can be obtained as follow:
Mass of compound = 7.546 g
Mass of nitrogen (N) = 1.957 g
Mass of Oxygen (O) =?
Mass of O = (Mass of compound) – (Mass of N)
Mass of O = 7.546 – 1.957
Mass of O = 5.589 g
Finally, we shall determine the empirical formula of the compound. This can be obtained as follow:
Mass of nitrogen (N) = 1.957 g
Mass of oxygen (O) = 5.589 g
Divide by their molar mass
N = 1.957 / 14 = 0.14
O = 5.589 / 16 = 0.35
Divide by the smallest
N = 0.140 / 0.14 = 1
O = 0.35 / 0.14 = 2.5
Multiply through by 2 to express in whole number
N = 1 × 2 = 2
O = 2.5 × 2 = 5
The empirical formula of the compound is N₂O₅.
Answer:
Explanation:
Hello there!
In this case, according to the given chemical reaction, it is possible for us to use the 1:2 mole ratio of nitrogen to ammonia to calculate the moles of the latter that are produced when reacting 3.15 moles of the former with hydrogen as shown below:
Thus, by solving the equation we obtain:
Best regards!
<span>A homogeneous mixture that does not settle out upon standing but will reflect light is
a. an element.
b. a colloid.
c. a suspension.
d. solid.
e. hydrated.
I think the answer is A</span>
Answer:
atoms are genetic so they are all different because they all have different parents (gens)
Answer:
180 mmHg
Explanation:
Total volume of gases = 20% + 80%= 100%
Total pressure of gases = 900 mm Hg
Note that partial pressure of a gas = mole fraction × total pressure
Mole fraction of oxygen = 20/100
Hence partial pressure of oxygen= 20/100 × 900 mm Hg
partial pressure of oxygen= 180 mmHg