Answer:
CaCN₂
Explanation:
A compound of calcium, carbon and nitrogen CaₐCₓNₙ in oxygen will burning producing:
CaₐCₓNₙ + O₂ → aCaO + xCO₂ + nNO₂
Moles of the oxides CaO, CO₂, NO₂ are:
CaO: 3.106g ₓ (1 mole / 56.08g) = <em>0.0554 moles of CaO = moles of Ca</em>
CO₂: 2.439g ₓ (1mole / 44g) = <em>0.0554 moles CO₂ = moles C</em>
NO₂: 5.097g ₓ (1mole / 46g) = <em>0.111 moles NO₂ = moles N</em>
Empirical formula is the chemical formula that represents the simplest ratio of elements in a compound.
Having as basis 0.0554 moles (The lower number of moles):
0.0554 moles Ca / 0.0554 = 1 Ca
0.0554 moles C / 0.0554 = 1 C
0.111 moles N / 0.0554 = 2N
Thus, the compound CaₐCₓNₙ has as empirical formula:
Ca₁C₁N₂ = <em>CaCN₂</em>
To make everything easier to convert so everything universal
Answer:
M = 35 g/mol
Explanation:
Given data:
Density = 2.5 g/L
Pressure = 1.8 atm
Temperature = 30°C (273.15 +30 = 303.15 K)
Molar mass = ?
Solution:
d = PM/RT
M = dRT/P
M = 2.5 g/L × 0.0821 atm.L/mol.K × 303.15 K / 1.8 atm
M = 62.22 atm. g/mol/ 1.8 atm
M = 35 g/mol
Answer:
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