First solve the moles of oxgen present in the compound
mol O = 6.93 g O ( 1 mol O / 16 g O )
mol O = 0.43 mol H
then solve the moles of hydrogen present
mol H = ( 7.36 - 6.93) g H ( 1 mol H / 1 g H)
mol H = 0.43 mol H
so the O and H are in the same mole content so the molecular formula would be OH, but the molar mass will not satisfy. so the answer would be
H2O2
Lose 1 electron
It will give it to an atom with more electrons. For example, Lithium (which has 1 valence electron) would give it to an atom that has more than 4 valence electrons
Answer: Compounds having the same empirical formula are:
Explanation:
Empirical formula tells us about the proportion of the elements present in the compound but it do not tells us about the actual numbers of atoms of the elements present in the compound.
In given empirical formula that is proportion of C:H:O = 1:2:1
In the proportion of C:H:O =2:4:2= 1:2:1
In the proportion of C:H:O =3:6:3= 1:2:1
In the proportion of C:H:O =1:2:2= 1:2:2
In the proportion of C:H:O =5:10:5= 1:2:1
In the proportion of C:H:O =6:12:6= 1:2:1
Compounds having the given empirical formula are:
Q = mCΔT
Q is heat, m is mass, C is specific heat, and ΔT is change in temp
First, find how much energy you need to raise the heat to 100C, or the boiling point
Q = (50g)(4.18)(75 degrees) = 15675 J or 15.675 kJ
Then you need 40.7 kJ extra for each mole of water to evaporate it
If you have 50 grams of water and there are 18 grams per mol
50g / 18g = 2.8 moles x 40.7 = 113 kJ extra
15.675 + 113 kJ = 128.7 kJ required
Answer:
955980 j
Explanation:
Given data:
Mass of water = 423 g
Temperature = 100°C
Amount of energy required = ?
Solution:
For one gram of water heat of energy required to convert it into vapors is 2260 j/g.
Amount of heat required for 423 g.
423 g × 2260 j/g = 955980 j
The amount of energy released when one gram steam is condensed into water is -2260 j.
For 423 g water vapor to condensed energy released.
423 g × -2260 j/g = -955980 j