Answer:
In comparison to Part 1 of this experiment, we observed similar reactions when determining the make up of our unknown. When testing for Mn2+ we observed a color change that resulted in a darker brown/red color, when testing for Co2+ we observed the formation of foamy bubbles but we could not conclude that a gas had formed, when testing for Fe3+ the result was a liquid red in color, when testing for Cr3+ we observed no change, when testing for Zn2+ we observed the formation of a pink/red liquid, when testing for K+ we observed the formation of a precipitate, when testing for Ca2+ we observe the formation of a precipitate. Sources of error may have occurred when observing whether or not an actual reaction had taken place or not, using glassware that wasn't fully cleaned, or the accidental mix of various other liquids in the lab
Explanation:
Answer:
The rate law cannot be defined based on just the formula given.
Explanation:
In the world of chemical kinetics there are four major concepts that are used to define the speed of a reaction. These are Rate Averaging, Equation Stoichiometry, Experimental Rate Laws and Integrated Rate Laws for Orders of Reaction. Each topic requires a reference reaction that has been defined in terms of the definition of reaction rates whose data can be applied to the expression ...
Rate = ΔConcentration/Δtime
If you will provide a balanced equation then empirical relationships can be presented that describe the consumption rate of reactants and/or the formation products. For example:
Given Equation 2NO₂(g) => 2NO(g) + O₂(g) and the measured rate of at least one component of the reaction, the following rate relationships can be defined:
Δ[NO₂(g)]/Δt = Δ[NO(g)]/Δt (Since coefficients are equal then the relationship is 1:1),
Δ[NO₂(g)]/Δt =2· Δ[O₂(g)]/Δt and
Δ[NO(g)]/Δt =2· Δ[O₂(g)]/Δt
Experimental Rate Law is based upon experimental observations of rxn rates as a function of molar concentration changes. The kinetic data is examined for 'Order of Rxn' and applied to the empirical rate law to obtain the numerical rate law.
Empirical Rate Law
Rate = k[NO₂(g)]ᵃ
k = rate constant
a = order of reaction
both are determined from experimentally observing rxn rate as a function of changing concentration of reactants.
Answer:
Trend in ionic character of bonds: Cs-F > Si-C > Br-Cl > Cl-Cl
(most) (least)
Explanation:
We know that, percentage ionic character of a bond is proportional to electronegativity difference between two constituting atoms.
Atom Electronegativity
Cs 0.7
F 4.0
Cl 3.0
Br 2.8
Si 1.8
C 2.5
Bond Electronegativity difference
Cs-F 3.3
Cl-Cl 0.0
Br-Cl 0.2
Si-C 0.7
So trend in ionic character of bonds:
Cs-F > Si-C > Br-Cl > Cl-Cl
(most) (least)
I would say that it sounds like you are an alchemist as during the 1500's at least they tried to turn base metals like Pb or lead into Au or gold. While this is not possible, their experiments gave rise to the science and techniques of metallurgy and assaying as confirmed by the great first mine geologist, Georgius Agricola in the 1500's,
Answer:
2.765amu is the contribution of the X-19 isotope to the weighted average
Explanation:
The average molar mass is defined as the sum of the molar mass of each isotope times its abundance. For the unknown element X that has 2 isotopes the weighted average is defined as:
X = Mass X-19 * Abundance X-19 + MassX-21 * Abundance X-21
The contribution of the X-19 isotope is its mass (19.00 amu) times its abundance (14.55% = 0.1455). That is:
19.00amu * 0.1455 =
2.765amu is the contribution of the X-19 isotope to the weighted average