Question

The following initial rate information was collected at
25^{o}C for the following reaction:

2H_{2(g)} + 2NO_{(g)} --> N_{2(g)} +
2H_{2}O_{(g)}

H_{2}]_{0} (M) |
[NO]_{0} (M) |
Initial Rate (M/min) |

0.0010 | 0.0020 | 1.2 x 10^{-4} |

0.0010 | 0.0030 | 1.8 x 10^{-4} |

0.0020 | 0.0020 | 4.8 x 10^{-4} |

Determine the overall order of the reaction and present you answer in numeric form (i.e. 0, 1, 2 etc).

Answer #1

Given reaction is A + B -----------> C + D

rate = k [A]^{m} [B]^{n} k = rate
constant

From trial 1,

1.2 x 10^{-4} = k [0.001]^{m}
[0.002]^{n} ------- Eq (1)

From trial 2,

1.8 x 10^{-4} = k [0.001]^{m}
[0.003]^{n} --------Eq (2)

From trial 3,

4.8 x 10^{-4} = k [0.002]^{m}
[0.002]^{n} --------Eq (3)

Do Eq(2)/Eq(1),

(1.8 x 10^{-4} /1.2 x 10^{-4} ) = (k/k)
(0.001/0.001)^{m} (0.003/0.002)^{n}

1.5 = 1^{m} x 1.5^{n}

1.5 = 1 x 1.5^{n}

Therefore, n =1

Do Eq(3)/Eq(1),

(4.8 x 10^{-4} /1.2 x 10^{-4} ) = (k/k)
(0.002/0.001)^{m} (0.002/0.002)^{n}

4 = 2^{m} x 1^{n}

Substitute n=1,

4 = 2^{m} x 1

4 = 2^{m}

2^{2} = 2^{m}

2= m

m = 2

Therefore, m= 2, n= 1

Then,

overall order of the reaction = m + n = 2 +1 =
**3**

Consider the following reaction:
2NO(g)+2H2(g)→N2(g)+2H2O(g).
If the rate constant for this reaction at 1000 K is
6.0×104M−2s−1, what is the reaction rate when [NO]=
2.90×10−2M and [H2]=
1.80×10−2M?
Express your answer using two significant figures.
rate =
M/s
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Part C
What is the reaction rate at 1000 K when the concentration of NO
is increased to 0.14 M, while the concentration of H2 is
1.80×10−2M?
Express your answer using two significant figures.

Consider the following reaction: 2NO(g)+2H2(g)→N2(g)+2H2O(g)
What is the reaction rate at 1000 K when the concentration of NO is
increased to 0.11 M, while the concentration of H2 is 1.50×10−2
M?
and If a solution containing 30.0 g of a substance reacts by
first-order kinetics, how many grams remain after three
half-lives?
and lastly The isomerization of
methylisonitrile to acetonitrile CH3NC(g)→CH3CN(g) is first order
in in CH3NC. The half-life of the reaction is 5.20 × 101 s at 545
K....

The experimentally determined rate law for the reaction
2NO(g)+2H2(g)→N2(g)+2H2O(g) is
rate=k[NO]2[H2].
Part A
What are the reaction orders in this rate law?
Enter your answers numerically separated by commas.
nNO, nH2 =
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Part B
Would the reaction rate increase more if we double the
concentration of NO or the concentration of H2?
A) The reaction rate will increase more if we double the
concentration of NO.
B) The reaction rate will increase more if we double the...

The reaction 2NO(g)+ 2H2(g) ---> N2(g)+ 2H2O(g)
was studied at 904 °C, and the data in the table were
collected.
Reaction Concentration (mol/L)
Rate of Appearance of N2
[NO]
[H2]
(mol/L·s)
0.498
0.122
0.191
0.249
0.122
0.0478
0.249
0.244
0.0956
0.125
0.488
0.0482
A) Determine the order of the reaction for each
reactant.
reaction order in [NO] = ____
reaction order in [H2] = ____
B) Write the rate equation for the
reaction.
(Use k for the rate constant.)
Rate...

The rate law for the reaction: 2H2+2NO--->N2+2H2O is
rate=k[H2][NO]^2. Which of the follwing mechanisms can be ruled out
on the basis of the observed rate expression? PLEASE EXPLAIN
Mechanism 1: H2+NO--->H2O+N (slow) / N+NO----->N2+O (fast)
/ O+H2----> N2+O (fast)
Mechanism 2: H2+2NO---->N2O+H2O (slow) / N2O+H2---->N2+H2O
(fast)
Mechanism 3: 2NO<----->N2O2 (fast equilibrium) /
N2O2+H2------>N2O+H2O (slow) / N2O+H2------>N2+H2O (fast)
PLEASE EXPLAIN WHY.

Using the information below determine the change in enthalpy for
the following reaction:
2NO(g) + 5 H2(g) → 2NH3(g) +
2H2O(l)
H2(g) + ½ O2(g) →
H2O(l)
∆H°= -285.8kJ
N2(g) + O2(g) →
2NO(g)
∆H°= +180.5 kJ
2NH3(g) → N2(g) +
3H2(g)
∆H°= + 92.22 kJ
please explain step by step! thanks!

For the reaction: 2H2O(g) ⇌ 2H2(g) + O2(g) KC = 2.40 x 10-3 at a
given temperature. At equilibrium, it is found that [H2O] = 0.294 M
and [H2] = 1.80 x 10-2 M. If the reaction is run in a 5.50 L
container, how many moles of O2 are present at equilibrium?

Using the Information below determine the change in enthalpy for
the following reaction:
2NO (g) + 5H2
(g)!2NH3
(g) + 2H2O
(l)
H2 (g) + 1⁄2O2 (g)!H2O (l) ΔH° = -285.8 kJ
N2 (g) + O2 (g)!2NO (l) ΔH° = +180.5 kJ
2NH3 (g)!N2 (g) + 3H2 (g)ΔH° = +92.22 kJ
a)-197.52 kJ
b)-241.7 kJ
c)-483.3 kJ
d)-659.88 kJ
e)-844.3 kJ
please show me which equation is first second and thrid and
reason why? i may be taking the wrong...

The following reaction establishes equilibrium at 2000K:
N2(g) + O2(g) ⇌ 2NO(g) where
Keq = 4.1 x 10-4
If the reaction began with 0.150 M of N2 and 0.150 M
of O2, the equilibrium concentration of NO would be

Consider this initial-rate data at a certain temperature for the
reaction described by:
2NOCl(g) yields 2NO(g) + Cl2(g)
NOCl
Intl. Rate of Form. of Cl2
(M)
.600
1.46 x 10^-5
.750
2.28 x 10^-5
.900
3.28 x 10^-5
Determine the value and units of the rate constant.
k=

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