43.56 grams of are produced if 16g of CH4 reacts with 64g of O2.
Explanation:
Balance equation for the reaction:
CH4 + 2O2⇒ CO2 +2H2O
Data given : mass of CH4 =16 grams atomic mass = 16.04 grams/mole
mass of water 36 gram atomic mass = 18 grams/moles
mass of CO2=? atomic mass = 44.01 grams/mole
number of moles = 
equation 1
number of moles in CH4
n = 
= 0.99 moles
Since combustion is done in presence of oxygen hence it is an excess reagent and methane is limiting reagent so production of CO2 depends on it.
From the equation
1 mole of CH4 gave 1 mole of CO2
O.99 moles of CH4 will give x moles of CO2
= 
x = 0.99 moles of carbon dioxide
grams of CO2 = number of moles x atomic mass
= 0.99 x 44.01
= 43.56 grams of CO2 is produced.
So first find the moles of the H₂SO₄: Mass = Moles x RFM
so mass = 5.25 x 98 = 514.5g of <span>H₂SO₄</span>
so to find how many Liters of solution use:
Volume = Density x Grams of solute (per kg +1000)
density = 1.266 x 514.5 +1000 = 1917.357kg/l
now use equation: Conc. = Moles / Volume of solution to find the conc.
Conc. = 5.25 x 1917.357 = 4.39Mol⁻¹
Hope that helps
First, you need to have a periodic table that contains the electronegativities values. once you have them, you just need to subtract the values of the atoms and each bond. I have attached a table with these values. also, it does not matter then order in which you subtract them because they are always positive values. even though you get negative values in your calculator, just make it positive.
H-S----> 2.1 - 2.5= 0.4
H-Cl---> 2.1 -3.0=0.9
H-O---> 2.1- 3.5= 1.4
H-F----> 2.1 - 4.0= 1.9
HF is the most polar because it has the highest electronegativity difference.
(1.632) (4.0 x 104)
= (1.632)(416)
=678.912
6.8* 10^2.
Not sure if it's the right sig figs.
