Answer:
It would Newton's third law.
Explanation:
Answer:
Li + Cl₂
Explanation:
left side of the arrow are reactants and right side of the arrow are products.
The atomic number is 6, you can also find out by the amount of electrons because, electrons and protons have the same charge.
Answer: The rates of production of 
is 
mol/Ls and 
is 0.0195 mol/Ls.
Explanation:
Rate with respect to reactants is shown by negative sign as the reactants are decreasing with time and Rate with respect to products is shown by positive sign as the products are increasing with time.
Rate of the reaction=![-\frac{1}{4}\frac{[d[PH_3]}{dt}=\frac{[d[P_4]}{dt}=\frac{1}{6}\frac{[d[H_2]}{dt}](https://tex.z-dn.net/?f=-%5Cfrac%7B1%7D%7B4%7D%5Cfrac%7B%5Bd%5BPH_3%5D%7D%7Bdt%7D%3D%5Cfrac%7B%5Bd%5BP_4%5D%7D%7Bdt%7D%3D%5Cfrac%7B1%7D%7B6%7D%5Cfrac%7B%5Bd%5BH_2%5D%7D%7Bdt%7D)
Rate of decomposition of 
Rate of production of 
Rate of production of 
Answer:
0.2990
Explanation:
All liquids intend to vaporize independent of the temperature if the pressure is higher enough. This pressure is called the vapor pressure. When it occurs, the liquid and the vapor phases will be in equilibrium, and so the fractions of the components of the liquids and the vapor can be calculated.
The molar fraction of the liquid (x) can be calculated by the composition, so, calling xc for cyclohexane, and ca for acetone:
xc = 1.90/(1.90 + 2.60) = 0.4222
xa = 1 - 0.4222 = 0.5778
The total pressure of the system (P) can be calculated by Dalton's Law:
P = Pc + Pa
Where Pc and Pa are the partial pressures of the components. The partial pressures can be calculated by the Raoult's Law:
Pc = xc*P°c
Pa = xa*P°a
Where P° is the vapor pressure, so:
P = xc*P°c + xa*P°a
P = 0.4222*97.6 + 0.5778*229.5
P = 137.8 torr
The molar fraction at the vapor phase (y) is the partial pressure divided by the total pressure:
yc = Pc/P
yc = (xc*P°c)/P
yc = (0.4222*97.6)/137.8
yc = 0.2990
