The activation energy of the first-order decomposition of N2O
into N2 and O is Ea= 250...
The activation energy of the first-order decomposition of N2O
into N2 and O is Ea= 250 kJ/mol. If the half-life of the reactant
is t1/2= 7.5*10^6 s at 673K, what will it be at 773K?
The decomposition of N2O to N2 and O2 is a first-order reaction.
At 730° C the half-life of the reaction is 3.58 × 103 min. If the
initial pressure of N2O is 5.50 atm at 730° C, calculate the total
gas pressure after one half-life. Assume that the volume remains
constant.
_____atm
Consider the first order reaction 2 N2O(g) ⟶ 2 N2 (g) + O2(g).
What will [N2O] be after 3 half lives when 0.25
moles N2O is placed in a 1.00-L reaction vessel?
(1) The activation energy, Ea, is the energy difference between the reactants and the products in a chemical reaction.(2) The activation energy is the energy barrier that must be overcome by reactants for a reaction to occur.(3) The frequency factor, A, in the Arrhenius equation relates to the number of collisions and the fraction of those collisions that have the proper geometry for a reaction to occur.
A.2 only
B.1 only
C.2 and 3
D.1 and 2
E.1 and...
The decomposition of benzene diazonium chloride C6H5N2Cl ->
C6H5Cl + N2 follows first order kinetics with a rate constant of
4.3 x 10-5 s-1 at 20 °C. If the initial partial pressure of
C6H5N2Cl is 0.088 atm, calculate its partial pressure after 10.0
hours. What is the half-life for this reaction?
1.Given the following data for the reaction A ® B, determine the
activation energy, Ea, of the reaction.
k (M/s)
T (K)
0.681
500
0.715
1,000
a.
2.05 ´ 10–2 kJ/mol
b.
405 J/mol
c.
6.90 J/mol
d.
48.7 J/mol
e.
9.95 kJ/mol
2. The mechanism for the reaction
2H2O2(aq) ®
2H2O(l) + O2(g) in the
presence of I–(aq) is proposed to be:
Step 1: H2O2(aq) +
I–(aq) ® H2O(l) +
OI–(aq)
Step 2: H2O2(aq) +
OI–(aq) ® H2O(l) +...
A particular reaction has an activation energy,
Ea, of 112 kJ/mol. If the rate
constant for the reaction is 0.00621 s
−1 at 452 °C, at what temperature(in°C)
would the rate constant be 0.145 s
−1?
The uncatalyzed decomposition of hydrogen peroxide (into water
and oxygen gas)
has an activation energy of 75.3 kJ mol-1.
a) By what factor will the rate constant increase if the
temperature is raised from
20°C to 30°C (i.e., what is the ratio of k30°C to k20°C)?
b) How much slower will the rate of decomposition be at 10°C
than 20°C (i.e., what
is the ratio of k10°C to k20°C)?
The activation energy for the decomposition of hydrogen iodide
is found to be 180 kJ mol–1 and the
rate constant for this reaction is reported to be 0.24 mol–1 L
min–1at 540 °C. What is k for this reaction
at 30 °C?
Please show all workings
Determine the activation energy in kJ/mol for a first order
reaction if its specific rate constant 8.30e-05 s-1 at
350.0 K and 3.25e+01 s-1 at 560.0 K.
Ea = ______ kJ/mol