what reaction type is
Cu2+ + OH- ---> Cu(OH)2
CuSO4 x 5H2O ----> CuSO4
CuSO4 ------> CuSO4 x 5H2O
NH4Cl -----> NH3 + HCl
Reaction Type Options are:
1. Combination, Synthesis or Formation Reaction
2. Decomposition Reaction
3. Single Displacement or Single Replacement Reaction
4. Double Displacement or Double Replacement Reaction
In: Chemistry
Is the ionic compound CaCO3 soluble or insoluble, and does each of its ions tend to be soluble?
a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble
Is the ionic compound NaNO3 soluble or insoluble, and does each of its ions tend to be soluble?
a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble
Is the ionic compound AgBr soluble or insoluble, and does each of its ions tend to be soluble?
a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble
Is the ionic compound (NH4)3PO4 soluble or insoluble, and does each of its ions tend to be soluble?
a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble
Classify the solution properties of 1.0 M acetic acid.
a. Strong electrolyte b. Weak electrolyte c. Non-electrolyte d. Pure liquid
Please Show Work
In: Chemistry
How can the Van Der Waals equation of state be used to determine whether a substance will be a solid, liquid or gas at a certain temperature and pressure?
In: Chemistry
Write a chemical reaction and a few words to explain why the pH of the formic acid buffer above goes up only tenths of a pH unit (from about 3.6 to about 3.7 pH units) when a few drops of 0.10 M NaOH solution are added to it, instead of going up much more to about pH=10. {Note that if the same amount of NaOH were added to 20 mL of 0.00025 M HCl (which also has pH=3.6), the pH would go up to about pH=10. Explain qualitatively – no calculation is needed.}
In: Chemistry
For the reaction show below determine the rate law.
CH3COCH3 + Br2 → CH3COCH2Br + HBr(aq)
The bromination of acetone, an organic solvent, is catalyzed by an acid. The rate of disappearance of bromine was measured for several different concentrations of the reactants including the catalyst, H+. Therefore, the catalyst will appear in the rate law, but not in the overall reaction. The following data were obtained:
[CH3COCH3] [Br2] [H+] Initial Rate (mol/L s)
0.30 0.05 0.05 5.7 x 10-5
0.30 0.10 0.05 5.7 x 10-5
0.30 0.05 0.10 11.7 x 10-5
0.40 0.05 0.05 7.6 x 10-5
Calculate the rate law for this reaction: rate = k [CH3COCH3][ ] [Br2][ ] [H+][ ]
In: Chemistry
Post Lab Questions:
A perfect percent yield would be 100%. Based on your results, describe your degree of accuracy and suggest possible sources of error.
What impact would adding twice as much Na2CO3 than required for stoichiometric quantities have on the quantity of product produced?
Determine the quantity (g) of pure CaCl2 in 7.5 g of CaCl2•9H2O.
Determine the quantity (g) of pure MgSO4 in 2.4 g of MgSO4•7H2O.
Conservation of mass was discussed in the background. Describe how conservation of mass (actual, not theoretical) could be checked in the experiment performed.
Based on these findings:
Data Table 1. Stoichiometry Values
|
Initial: CaCl2•2H2O (g) |
.68 |
|
Initial: CaCl2•2H2O (moles) |
.0068 |
|
Initial: CaCl2 (moles) |
.00368 |
|
Initial: Na2CO3 (moles) |
.0012 |
|
Initial: Na2CO3 (g) |
.12 |
|
Theoretical: CaCO3 (g) |
.68 |
|
Mass of Filter paper (g) |
1g |
|
Mass of Filter Paper + CaCO3 (g) |
1.7g |
|
Actual: CaCO3 (g) |
.72g |
|
% Yield: |
103 |
In: Chemistry
What is cyanoarylate ester? What is it used for? What is the history behind it?
In: Chemistry
How many grams of AgBr will dissolve in 1.0 L of water containing a Br- concentration of 0.050 M? Ksp= 5.0 * 10^-13
In: Chemistry
Calculate the ΔG°rxn using the following information. 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔH°f(kJ/mol) -20.6 296.8 -241.8 S°(J/mol∙K) 205.8 205. 248.2 188.8 ΔG°rxn = ?
| +676.2 kJ | |
| +108.2 kJ | |
| -466.1 kJ | |
| +196.8 kJ | |
| -147.1 kJ |
In: Chemistry
Propose a buffer system using ascorbic acid. Explain how this solution can protect against acids and bases, specifically.
In: Chemistry
Compare the deltaS fusion with the deltaS vaporization for water. Are they reasonable in terms of the relative disorder of the states of matter?
deltaH fusion= 6.10 kJ/mol and deltaH vap= 40.7 kJ/mol
In: Chemistry
Write balanced net ionic equations for the following reactions in basic solution:
H2O2(aq)+Cr2O2−7(aq)⟶O2(g)+Cr3+(aq)
Express your answer as a balanced net ionic equation. Identify all of the phases in your answer.
In: Chemistry
a. Assuming that glucose and water form an ideal solution, what is the partial pressure of water at 20o C of a solution of 1.00 g of glucose (mol wt 180 g/mol) in 100 g of water? The vapor pressure of pure water is 2338 Pa at 20o C.
b. What is the osmotic pressure, in Pa, of the solution in part (a) versus pure water?
c. What would be the osmotic pressure, in Pa, of a solution containing both 1.00 g of glucose and 1.00 g of sucrose (mol wt 342) in 100 g of water at 20o C?
In: Chemistry
What is the pH of 50 ml of a 0.10M weak acid (Ka =1.0x10-5) plus 50ml water?
What is the pH of 50 ml 0.010M weak base plus 100ml water ? Kb =1.0x10-5.
What is the pH of a solution, which is 0.10M in a weak acid, HA and 0.2M in NaA? Ka =1.0x10-5In: Chemistry
Electronic configurations follow from the principle quantum numbers n, l, m, and s. What is the relationship with n and the periodic table? What is the relationship with n and the number of valance electrons? The ‘l ’ quantum number designates the type of orbital. What is an orbital? Do electrons have to stay in their designated orbital? The ‘m’ quantum number gives the degeneracy of the orbital type. Is there a difference in the px and py orbitals? Why does the spinning of the two electrons sharing an orbital have to be opposite. Are electrons really spinning?
In: Chemistry