What is a disruption or change that is happening to the body that causes it to sweat ?
1 answer:
You might be interested in
Answer:
m1/6 ( c )
Explanation:
since all the balls starts having the same momentum after the two collisions we will apply the principal of conservation of energy
After first collision
m1v = m1v1 + m2v2 --- ( 1 )
After second collision
m2v2 = m2v2 + m3v3 ---- ( 2 )
combining equations 1 and 2
m1v = m1v1 + m2v2 + m3v3 ----- ( 3 )
All balls moving at the same momentum ( p ) = m1v1 = m2v2 = m3v3
note ; 3p = m1v ∴ m3 = ----- ( 4 )
applying conservation of energy
3v = v1 + v2 + v3 ------- ( 5 )
also 3m1v1 = m1v = v1 = v/3 =
v2 + v3 = 8/3 v ----- ( 6 )
next eliminate V3 for equation 6 by applying conservation of energy and momentum
m1 = 2m2 ------ ( 7 )
now using p1 = p2 = m1v1 = 1/2 m1v1 hence v2 = 2v1 where v1 = 1/3 v
hence ; v2 = 2/3 v ------- ( 8 )
solving with equation 6 and 8
v3 = 2v ------ ( 9 ) ∴ v/v3 = 1/2 ---- ( 10 )
solving with equation 9 and 10
m3 = m1/3 * 1/2 = m1/6
Molecular formulas:
- CH₂O;
- C₂H₄O₂;
- C₆H₁₂O₆.
The empirical formula of a compound tells only the ratio between atoms of each element. The empirical formula CH₂O indicates that in this compound,
- for each C atom, there are
- two H atoms, and
- one O atom.
The molecular weight (molar mass) of the molecule depends on how many such sets of atoms in each molecule. The empirical formula doesn't tell anything about that number.
It's possible to <em>add</em> more of those sets of atoms to a molecular formula to increase its molar mass. For every extra set of those atoms added, the molar mass increase by the mass of that set of atoms. The mass of one mole of C atoms, two mole of H atoms, and one mole of O atoms is .
- CH₂O- 30.0 g/mol;
- C₂H₄O₂- 30.0 + 30.0 = 2 × 30.0 = 60.0 g/mol;
- C₃H₆O₃- 30.0 + 30.0 + 30.0 = 3 × 30.0 = 90.0 g/mol.
It takes one set of those atoms to achieve a molar mass of 30.0 g/mol. Hence the molecular formula CH₂O.
It takes two sets of those atoms to achieve a molar mass of 60.0 g/mol. Hence the molecular formula C₂H₄O₂.
It takes sets of those atoms to achieve a molar mass of 180.0 g/mol. Hence the molecular formula C₆H₁₂O₆.