The decomposition of XY is second order in XY and has a rate constant of 6.94×10−3 M−1⋅s−1 at a certain temperature.
If the initial concentration of XY is 0.160 M , how long will it take for the concentration to decrease to 6.00×10−2 M ? Express your answer using two significant figures.
If the initial concentration of XYXY is 0.050 MM, what is the concentration of XYXY after 500 ss ?
Express your answer using two significant figures.
In: Chemistry
Reaction enthalpy for ethanol oxidation, C2H5OH+3O2 -> 2CO2 + 3H2O is 1257 kJ/mole.
Energy content per mol fuel ______kJ Energy content per gram fuel = ____________ kJ
Energy released per mol CO2 formed ________ kJ Energy released per mol O2 consumed= ______ kJ
Moles of CO2 formed per 1000 kJ energy released ___________
In: Chemistry
a) Explain oxidative addition and carbonyl insertion reactions in organometallic chemistry with
appropriate examples.
b) Explain pictorially the σ- and π-bonding in metal-carbonyl compounds and comment on the synergistic effect.
c) What are the experimental evidences and how they support synergistic effect in metal carbonyl bonding?
In: Chemistry
Explain the sublimation and vaporization processes. How does the condensation process relate to vaporization and how does deposition relate to sublimation? Give an example of each process
In: Chemistry
1. Use this data table for the bromination of acetone to answer the following questions;
|
Experiment |
[CH3COCH3] (M) |
[Br2] (M) |
[H+] (M) |
Rate (M s-1) |
|
1 |
0.3 |
0.05 |
0.05 |
0.000057 |
|
2 |
0.3 |
0.10 |
0.05 |
0.000057 |
|
3 |
0.3 |
0.05 |
0.10 |
0.000120 |
|
4 |
0.4 |
0.05 |
0.20 |
0.000310 |
|
5 |
0.4 |
0.05 |
0.05 |
0.000076 |
a) Determine the reaction order with respect to each of the three reactants and write the rate law.
b) What is the value of the rate constant including proper units?
In: Chemistry
For each of the transition metal complex ions
(a) [Ti(NH3)6]2+
(b) [Cr(H2O)4(OH)2]1-
(c) trans–[Pt(CN)2(en)2]2+
(i) Draw the structure of the transition metal complex ion. Show
the charge on the
complex.
(ii) Determine the number of d electrons.
(iii) Draw the ground state arrangement of the d electrons in the
ground state.
(iv) Calculate the LFSE (in units of Δo or ΔT) for each
complex.
In: Chemistry
1) A) Draw the dipeptide Y-C at pH 7 and clearly label the peptide bond to be broken in the presence of chymotrypsin.
B) Draw the five-step mechanism for the chymotrypsin clevage of the dipeptide.
C) Label the transition state each time it is formed.
D) What mechanism is used to describe this bisubstrate reaction?
In: Chemistry
1. For the reaction: 2Mg(s) + O2(g) → 2MgO Calculate the percent yield if 10g of Mg and 15g of O2 react, and 15.0g MgO was actually obtained.
2. For the reaction: H2(g) + Cl2(g) → HCl(g) (is this balanced?) calculate the mass, in grams of Hydrogen Chloride produced when H2 reacts with 25.0g Cl2.
In: Chemistry
calculate the mass percent of oxalate ion in H2C2O4*2H2O and (NH4)2C2O4*H2O
In: Chemistry
In: Chemistry
3. Which of the following is an ortho and
para-director and a deactivator? (10 pts)
a. —NHCOCH2CH3 b. —CH2CH2CH3
c. —CH2CCl3 d. —COCH2CH2Cl
e. none of the above
In: Chemistry
A Photomultiplier tube can detect a single photon, but a photodiode cannot. Why is this? As part of your answer sketch the main components of both devices and describe how they work.
In: Chemistry
A buffer solution contains 0.29 mol of phenol
(HC6H5O) and 0.75 mol of sodium phenoxide
(NaC6H5O) in 5.20 L.
The Ka of phenol (HC6H5O) is
Ka = 1.3e-10.
(a) What is the pH of this buffer?
pH = ?????????????
(b) What is the pH of the buffer after the addition of 0.06 mol of
NaOH? (assume no volume change)
pH = ????????????
(c) What is the pH of the original buffer after the addition of
0.59 mol of HI? (assume no volume change)
pH = ????????????
In: Chemistry
which of the following yields a buffer solution when equal volumes of the two solutions are mixed? A.) 0.10M HCl and 0.10M NaCl B.) 0.15M HNO3 and 0.15M NaNO3 C.) 0.10M HF and 0.10M NaF D.) 0.10M HClO4 and 0.10M NaClO4 E.) 0.15M HBr and 0.15M NaBr
In: Chemistry
When 5.00 g of acetone (C3H6O) burns in air, carbon dioxide gas and liquid water are formed. Enough heat is liberated to increase the temperature of 1.000 kg of water from 25.0◦C to 61.8◦C. The specific heat of water is 4.18 J/g-◦C
1. How many kJ of heat are liberated by the combustion described?
2. How many grams of acetone must be burned to liberate 5.00 kJ?
3. Write the thermochemical equation for the combustion of acetone.
4. What is ΔH◦f for acetone?
5. What volume of oxygen at 25◦C and 747 mm Hg is consumed when 25.00 kJ of heat are liberated?
In: Chemistry