Question

For a Reaction that has positive activation energy, would you expect increasing the temperature to increase or decrease the reaction rate? Please explain your answer in using "rate=K[A]^x[B]^y" and "K=Ae*-Ea/rT"

Answer #1

**we know that**

**K = Ae^-(Ea / RT)**

**ln K = ln A - (Ea / RT)**

**now**

**at two different temperatures**

**ln K1 = ln A - ( Ea / RT1)**

**ln K2 = ln A - (Ea / RT2)**

**solving we get**

**ln ( K2 / K1) = (Ea / R) ( 1/T1 - 1/T2)**

**given**

**Ea = +ve**

**also**

**the temperature is increased**

**so**

**T2 > T1**

**1/T2 < 1/ T1**

**1/T1 - 1/T2 > 0**

**also**

**Ea > 0**

**so**

**ln ( K2 / K1) > 0**

**so**

**K2 > K1**

**so**

**the rate constant has increased**

**now**

**rate = K [A]^x [B]^y**

**as K increased**

**the rate also will increase**

**so**

**the reaction rate is increased as the temperature is
increased**

There are several factors that affect the rate of a reaction.
These factors include temperature, activation energy, steric
factors (orientation), and also collision frequency, which changes
with concentration and phase. All the factors that affect reaction
rate can be summarized in an equation called the Arrhenius
equation:
k=Ae−Ea/RT
where k is the rate constant, A is the
frequency factor, Ea is the activation energy,
R=8.314 J/(mol⋅K) is the universal gas constant, and
T is the absolute temperature.
__________________________________________________
A certain...

explain a procedure/analysis to measure activation energy (Ea)
experimentally by using the Arrhenius expression for the
temperature dependence of the rate constant k
k(T)=Ae-Ea/RT

The energy of activation for the reaction 2 HI → H2 + I2 is 180.
kJ·mol−1 at 556 K. Calculate the rate constant using the equation k
= Ae^(−Ea/RT). The collision diameter for HI is
3.5 ✕ 10−8 cm. Assume that the pressure is 1.00 atm.

A certain reaction has an activation energy of 60.0 kJ/mol and a
frequency factor of A1 = 2.80×1012 M−1s−1 . What is the rate
constant, k, of this reaction at 30.0 ∘C ?
I tried k = Ae^(-Ea/RT) but it's giving me 1.26E2 M^-1s^-1 which
is wrong on my online homework, I did convert C to K and kJ/mol to
J.

a.)A certain reaction has an activation energy of 25.10 kJ/mol.
At what Kelvin temperature will the reaction proceed 7.00 times
faster than it did at 289 K?
b.A certain reaction has an enthalpy of ΔH = 39 kJ and an
activation energy of Ea = 51 kJ. What is the activation energy of
the reverse reaction?
c.)At a given temperature, the elementary reaction A<=> B in
the forward direction is the first order in A with a rate constant
of...

The sign of delta H is positive. Increasing the temperature
will:
A. Increase extent and reaction rate
B. Decrease extent and reaction rate
C. decrease extent and increase reaction rate
D. increase extent and decrease reaction rate

A certain reaction has an activation energy of 31.40 kJ/mol. At
what Kelvin temperature will the reaction proceed 6.50 times faster
than it did at 293 K?
Use the Arrhenius equation
ln (k2/k1) = Ea/R [(1/T1)-(1/T2)]
Where R=8.3145 J/(molxK)

The Arrhenius equation shows the relationship between the rate
constant k and the temperature T in kelvins and is typically
written as k=Ae−Ea/RT where R is the gas constant (8.314 J/mol⋅K),
A is a constant called the frequency factor, and Ea is the
activation energy for the reaction. However, a more practical form
of this equation is lnk2k1=EaR(1T1−1T2) which is mathmatically
equivalent to lnk1k2=EaR(1T2−1T1) where k1 and k2 are the rate
constants for a single reaction at two different absolute...

A. The Arrhenius
equation shows the relationship between the rate constant
k and the temperature T in kelvins
and is typically written as
k=Ae−Ea/RT
where R is the gas constant (8.314 J/mol⋅K), A
is a constant called the frequency factor, and Ea
is the activation energy for the reaction.
However, a more practical form of this equation is
lnk2k1=EaR(1T1−1T2)
which is mathematically equivalent to
lnk1k2=EaR(1T2−1T1)
where k1 and k2 are the rate constants for a
single reaction at two different...

The
Arrhenius equation shows the relationship between the rate constant
k and the temperature Tin kelvins and is
typically written as
k=Ae−Ea/RT
where R is the gas constant (8.314 J/mol⋅K), Ais
a constant called the frequency factor, and Ea is
the activation energy for the reaction.
However, a more practical form of this equation is
lnk2k1=EaR(1T1−1T2)
which is mathmatically equivalent to
lnk1k2=EaR(1T2−1T1)
where k1 and k2 are the rate constants for a
single reaction at two different absolute temperatures
(T1and...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 2 minutes ago

asked 20 minutes ago

asked 32 minutes ago

asked 47 minutes ago

asked 53 minutes ago

asked 53 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago