Question

**1) Express your answer as a molecular
formula.**

a) Use the data below to calculate the heat of hydration of lithium chloride.

b) Calculate the heat of hydration of sodium chloride.

Compound |
Lattice Energy
(kJ/mol) |
ΔHsoln(kJ/mol) |

LiCl | -834 | -37.0 |

NaCl | -769 | +3.88 |

2)A certain reaction with an activation energy of 115 kJ/mol was
run at 485 K and again at 505 K . What is the ratio of *f*
at the higher temperature to *f* at the lower temperature?
**Express your answer numerically using one significant
figure. f505/f485=?**

**3)**The gas-phase reaction of NO with F2 to form
NOF and F has an activation energy of *E*a = 6.30 kJ/mol and
a frequency factor of *A* =
6.00×10^{8}*M*−1⋅s−1 . The reaction is believed to
be bimolecular:

NO(g)+F2(g)→NOF(g)+F(g)

What is the rate constant at 657 ∘C ?

4)Consider the following reaction:

2HBr(*g*)→H2(*g*)+Br2(*g*)

a)In the first 25.0 s of this reaction, the concentration of HBr dropped from 0.600 M to 0.458 M . Calculate the average rate of the reaction in this time interval.

b)If the volume of the reaction vessel in part (b) was 1.50 L, what amount of Br2 (in moles) was formed during the first 15.0 s of the reaction?

5)Consider the following reaction:

2N2O(*g*)→2N2(*g*)+O2(*g*)

a)In the first 14.0 s of the reaction, 1.7×10^{−2} mol
of O2 is produced in a reaction vessel with a volume of 0.360 L .
What is the average rate of the reaction over this time
interval?

b)Predict the rate of change in the concentration of N2O over
this time interval. In other words, what is Δ[N2O]/Δ*t*?

Answer #1

1) solution : the reation will be

a) Li^{+} + Cl ^{-} --> LiCl(s)
deltaH lattice =-834KJ /mole .........equation 1

LiCl (s) + aq --> LiCl(aq) Delta H solution = -37 J / mole......equation 2

Li^{+} + Cl ^{-} --> LiCl (aq) Hydration

So Delta H hydration = Equation 1 + equation 2 = -834 + (-37 ) =-871 KJ / mol

b) Na^{+} + Cl ^{-} --> NaCl(s)
deltaH lattice = -769KJ /mole .........equation 1

NaCl (s) + aq --> NaCl(aq) Delta H solution = 3.88J / mole......equation 2

Na^{+} + Cl ^{-} --> NaCl (aq) Hydration

So Delta H hydration = Equation 1 + equation 2 = - 769 + (+3.88 ) = - 765.12KJ / mol

2.

3.

Ea = 6.30 kJ/mol = 6.30X10^{3} J/mol

A = 6.00×10^{8} M^{−1}⋅s^{−1}

Temperature, T = 657^{o}C = 657 + 273

= 930 K

Rate constant ids given by the arhenious equation as:

K = A*e^{(- Ea/RT)}

K = 6.00X10^{8} *e^{(- 6300
/8.314*630)}

K = 6.00X10^{8} *e^{- 0.814793}

K = 6.00X10^{8} *0.442730

K = 2.6564X10^{8} M^{-1} s^{-1}

Constants | Periodic Table The gas-phase reaction of NO with F2
to form NOF and F has an activation energy of Ea = 6.30 kJ/mol and
a frequency factor of A = 6.00×108 M−1⋅s−1 . The reaction is
believed to be bimolecular: NO(g)+F2(g)→NOF(g)+F(g)
What is the rate constant at 537 ∘C ? Express your answer to
three significant digits with the appropriate units. For compound
units, place a multiplication dot between units (e.g.
J⋅mol−1⋅K−1).

The gas-phase reaction of NO with F2 to form NOF and F has an
activation energy of Ea = 6.30 kJ/mol and a frequency
factor of A = 6.00×108M−1⋅s−1 . The
reaction is believed to be bimolecular:
NO(g)+F2(g)→NOF(g)+F(g)
What is the rate constant at 695 ∘C ?
Express your answer to three significant digits with the
appropriate units. For compound units, place a multiplication dot
between units (e.g. J⋅mol−1⋅K−1).
(I got 2.74*10^8 M-1s-1 but it is wrong. I got a...

1. Consider the reaction 2N2O(g) ->
2N2(g) + O2(g)
A. (2) Express the reaction in terms of the change in the
concentration of each of the reactants and products.
B. (2) In the first 15 seconds of the reaction, 0.015 mol of
O2 is produced. What is the average rate of the reaction
during this time interval?

15.28
Consider the following reaction:
2 N2O(g) ? 2 N2(g)+O2(g)
A
In the first 13.0 s of the reaction,
1.6×10?2 mol of O2 is produced in a reaction
vessel with a volume of 0.400 L . What is the average
rate of the reaction over this time interval?
Express your answer using two significant figures.
B.
Predict the rate of change in the concentration of N2O over this
time interval. In other words, what is ?[N2O]?t?
Express your answer using two significant figures.

The decomposition of NO2(g) occurs by the
following bimolecular elementary reaction.
2 NO2(g) → 2 NO(g) +
O2(g)
The rate constant at 273 K is 2.3 ✕ 10-12 L/mol · s,
and the activation energy is 111 kJ/mol. How long will it take for
the concentration of NO2(g) to decrease from an
initial partial pressure of 4.0 atm to 2.4 atm at 451 K? Assume
ideal gas behavior.

The rate constant for the reaction below was determined to be
3.241×10-5 s–1 at 800 K. The activation energy of the reaction is
215 kJ/mol. What would be the value of the rate constant at
9.10×102 K? N2O(g) --> N2(g) + O2(g)
I'm having trouble calculating the rate constant with the
arrhenius equation that deals with two temps, could you show me the
step by step how to do this?

Consider the following reaction:
2 N2O(g) → 2 N2(g)+O2(g)
In the first 10.0 s of the reaction, 1.7×10−2 mol of O2 is
produced in a reaction vessel with a volume of 0.430 L . What is
the average rate of the reaction over this time interval?

Use the Born-Haber cycle, and the following data to
calculate the bond dissociation energy of F2.
Na(g) → Na+(g) + e-(g) ΔrH = IE1 =
500 kJ mol-1
Na(s) → Na(g) ΔsubH = 107 kJ
mol-1
F-(g) → F(g) + e-(g) ΔrH = EA1 = 329
kJ mol-1
Na(s) + 1/2 F2(g) → NaF(s) ΔfH =
-569 kJ mol-1
Na+(g) + F-(g) → NaF(s) ΔlattH =
-928 kJ mol-1

At elevated temperatures, in the absense of a catalyst, nitrous
oxide decomposes by a first order proces according the the
equation: 2N2O (g) --> 2N2 (g) +
O2 (g). From an experiment at 430 degrees Celsius,
k is found to be 3.8 x 10-5 s-1; at
700 degrees Celsius, k is found to be 1.0
s-1.
a. Using the two-point version of the linearized Arrhenius
equation, please find the activation energy (kJ/mol) for the
decomposition of N2O (g).
b. Given...

1)Use standard thermodynamic data (in the Chemistry References)
to calculate G at 298.15 K for the following reaction, assuming
that all gases have a pressure of 19.31 mm Hg. 2N2(g) +
O2(g)2N2O(g)
G = ? kJ/mol
2)Using standard thermodynamic data (linked), calculate the
equilibrium constant at 298.15 K for the following reaction.
C2H4(g) + H2O(g)CH3CH2OH(g)
K = ?
3) Calculate the temperature (in kelvins) at which the sign of
G° changes from positive to negative for the reaction below. This...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 31 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago