O1Fl2
1. Assume an 100g sample, so the percentage will stay the same
2. Covert each element into their molar mass
29.6/16.00=1.8 mols of O
70.4/19.00=3.7 mols of Fl
3. Divide both by the smallest value of mol
1.8/1.8=1 O
3.7/1.8=2 Fl
4. Write the empirical formula:
O1Fl2
Empirical formula is the simplest ratio of components making up the compound. the molecular formula is the actual ratio of components making up the compound.
the empirical formula is CH₂. We can find the mass of CH₂ one empirical unit and have to then find the number of empirical units in the molecular formula.
Mass of one empirical unit - CH₂ - 12 g/mol x 1 + 1 g/mol x 2 = 12 = 14 g
Molar mass of the compound is - 252 .5 g/mol
number of empirical units = molar mass / mass of empirical unit
= 
= 18 units
Therefore molecular formula is - 18 times the empirical formula
molecular formula - CH₂ x 18 = C₁₈H₃₆
molecular formula is C₁₈H₃₆
My guess on that molecule is nucleus , sorry if it’s not correct
iodine which should appear before tellurium and argon which should appear after potassium
There is a 3rd one: nickel should appear before cobalt
Answer:
8L of CO2
Explanation:
The equation for the reaction is given below:
2C2H2 + 5O2 —> 4CO2 + 2H2O
From the equation above,
5L of O2 produced 4L of CO2.
Therefore, 10L of O2 will produce = (10 x 4)/5 = 8L of CO2
Therefore, 8L of CO2 is produce