Empirical formula is the simplest ratio of whole numbers of components in a compound
calculating for 100 g of compound
C H O
mass 64.27 g 7.19 g 28.54 g
number of moles 64.27 g / 12 g/mol 7.19 g/1 g/mol 28.54 g / 16 g/mol
= 5.356 mol = 7.19 mol = 1.784 mol
divide by least number of moles
5.356 / 1.784 7.19 / 1.784 1.784 / 1.784
= 3.002 4.03 = 1.000
rounded off to nearest whole number
C - 3
H - 4
O - 1
empirical formula - C₃H₄O
mass of empirical formula = 12 g/mol x 3 + 1 g/mol x 4 + 16 g/mol x 1 = 56 g
molecular mass = 168.19 g/mol
molecular formula is the actual ratio of elements making up the compound
number of empirical units = molar mass of molecule / empirical mass
empirical units = 168.19 g/mol / 56 g = 3.00
there are 3 empirical units making up the molecular formula
molecular formula = 3 x C₃H₄O
molecular formula = C₉H₁₂O₃
10 HSiCl3+ 15 H2O→H10Si10O15+ 30 HCl
Explanation:
Step 1: To make Si equal on both sides. put 10 in front of HSiCl3
10 HSiCl3+ H2O →H10Si10O15+ HCl
Step 2: By putting 30 in front of HCl, Cl can be balanced
10 HSiCl3+ H2O →H10Si10O15+ 30 HCl
Step 3: Now, balance O by putting 15 in front of H2O
10 HSiCl3+ 15 H2O→H10Si10O15+ 30 HCl
Hence the balanced equation is:
10 HSiCl3+ 15 H2O→H10Si10O15+ 30 HCl
Answer:
the particles, molecules, and gas range from smallest to largest in the following order: electron < proton < atom <...
Answer:
149.6 grams
Explanation:
Mass in gram = molar mass * number of moles
Massof CO2 in gram = 44*3.4=149.6 grams
Reduction is only one half of the reaction of a redox (reduction-oxidation reaction). It is characterized by the reduction of oxidation number or the gain of electrons. So, you would expect the reaction to have moles of electrons in the reactant side to depict gaining of electrons. The reduction reaction is as follows:
<em>HNO₂ + e⁻ --> NO</em>
Why only 1 e-? Compute the oxidation number of N in the reactant side.
1+x+2(-2) = 0; x = +3
Then, compute the oxidation number of N in the product side.
x -2 = 0; x = +2
So, there is a difference of 1 electron. Hence, 1e-.
