The molecular formula for mustard gas is C₄H₈SCl₂
the molecular mass of mustard gas - 159.09 g/mol
atomic mass of H is 1 g/mol
The mass of H in 1 mol of compound - 1 x 8 = 8 g
this means that in 159.09 g of compound , 8 g of H present
mass percentage of hydrogen = 8 g/ 159.09 g x 100%
mass percentage of hydrogen = 5.03%
Li+ have<span> more</span> elements i think
Answer:
Equation: C3H8 + 5O2 = 3CO2 + 4H2O (already balanced)
a) If you start with 14.8 g of C3H8 and 3.44 g of O2, determine the limiting reagant
b) Determine the number of moles of carbon dioxide produced
c) Determine the number of grams of H2O produced
d) Determine the number of grams of excess reagant left
I think the answer is D no change. Though you add more CO2, but the pressure is not mentioned. If the pressure is constant and the reaction is already balanced, the H2O is also saturation and can not absorb more CO2.
Explanation:
Expression for the kinetic energy is as follows.
K.E = 
Now, total kinetic energy will be as follows.
K.E = 
= 
Since, this energy converts into electromagnetic radiation of wavelength 121.6 nm.
Relation between energy and photon is as follows.
Energy of photon = 
= 
= 
v = 
= 
m/s
Thus, we can conclude that atoms were moving at a speed of m/s before the collision.
