Please show me the work, how you get it. Thank you 6/ consider the reaction 2h2

Question

Please show me the work, how you get it. Thank you

6/ consider the reaction 2h2 + O2 ---> 2h2O. What is the ratio of the initial rate of appearance of water to the initial rate of disappearance of oxygen?

A/ 1:1

B/ 2:1

C/ 1:2

D/ 3:2

7/ consider the following rate law: Rate = K[A]^n [B]^m. How are the exponents n and m determined ?

A/ By using the balanced equation

B/ By using the subcripts for the chemical formulas

C/ By hypothesis

D/ By experiment

8/ the catalyzed pathway in a reaction mechanism has a _______ activation energy and thus causes a ______ reaction rate

A/ higher, lower

B/ higher, higher

C/ lower, higher

D/ Lower, lower

16/ the rate law for the reaction A + 3B ----> C +2D is Rate =K[A]^2[B]^3. The order of the reaction is ?

A/ 2

B/ 3

C/ 5

D/ 6

17/ A Solution is made by dissolving 500 grams of ammonium nitrate in enough water to make 2.50 liters of solution. Determine the molarity and write the appropriate units.

26/ which of the following is a conjugate acid/base pair?

A/ HCL/OCL-

B/ H2SO4/SO4^2-

C/ NH4+/ NH3

D/ H3O+/OH-

28/ A proton in an aqueous solution combines with a water molecule to form a

A/ H+

B/H3O+

C/ OH-

D/ OH2-

29/ which pair acts as bronsted – lowry bases in the equilibrium:

HCL + NH3 ---> <---- NH4+ CL-

A/ HCL and NH4+

B/ NH3 and CL-

C/ HCL and CL-

D/ NH3 and NH4+

31/ 2NO + H2 ----> N2O + H2O

experiment initial[NO] (mol/L) initial [H2] ( mol/L) rate ( mol/L*S)

1 6.4 x 10^-3 2.2 x 10^-3 2.6 x 10^-5

2 12.8 x 10^-3 2.2 x 10^-3 1.0 x 10^-4

3 6.4 x 10^-3 4.5 x 10^-3 5.1 x 10^-5

I/ write the rate law for this reaction

II/ Determine the rate constant for this reaction with the appropriate units/

III/ what is the order of this reaction?

36/ Write the equilibrium expression Kc for the reversible reaction:

2NO(g) + O2(g) -----> 2NO2(g)

37/Initially 2.0 moles of N2(g) and 4.0 moles of H2(g) were added to a 1.0-liter container and the following reaction then occurred:
3H2(g) + N2(g) 2NH3(g)
The equilibrium concentration of NH3(g) = 0.68 moles/liter at 700°C. Determine Kc at 700°C for the formation of ammonia

38/ For the reaction: H2(g) + Br2(g) ----> 2HBr(g) kp= 3.5 x 10^4 at 1495k

what is the value of Kp for the following reaction at 1495K.

I/ 1/2H2(g) + 1/2Br2(g) ----> HBr(g)

II/ 4HBr(g) -----> 2H2(g) + 2Br2(g)

41/ calculate the [H+] in a solution that has a pH of 11.70 at 25 celcius.

42/ Determine the pH of a solution at 25 celcius in which the [OH-] = 3.4 x 10^-5 M.

43/ Calculate the pH of a 0.250 M HNO3(aq) solution at 25 celcius.

44/ Determine the pH of a solution at 25 celcius if the pOH is 3.75.

45/ Determine the molarity of a solution prepared by adding 350 grams of potassium hydroxide to enough water to make 5.75 liters of solution.

47/ of the following, a 0.10M aqueous solution of __________ will have the highest boiling point.

A/ NACL

B/ AL(NO3)3

C/ K2CrO4

D/ Na2SO4

48/ Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction:

2NO2 -----> 2NO + O2

In a particular experiment at 300 celcius , [NO2] drops form 0.0100 M to 0.00650 M in 100 seconds. The rate of appearance of O2 for this period is _________ M/s.

A/ 1.8 x 10^-5

B/ 3.5 x 10^-5

C/ 7 x 10^-5

D/ 3.5 x 10^-3

E/ 7 x 10^-3

Explanation / Answer

6)1/2 RATE OF DISAPPEARENCE OF NO2 = RATE OF APPEARENCE OF O2   

(RATE OF DISAPPEARENCE OF NO2)/(RATE OF APPEARENCE OF O2) = 2/1

ANSWER IS B 2:1

7) D) BY EXPERIMENT

8) C) lower, higher

16) C) 5

SUM OF THE POWERS OF CONCENTRATION TERMS INVOLCED IN THE RATE LAW EXPRESSION IS CALLED AS ORDER OF THE REACTION.

17)

M= (wt.of ammonium nitrate)/(m,wt of ammonium nitrate*volume)

    = 500/(80.050*2.50)

= 2.49M

26) C) NH4^+ & NH3 BECAUSE ONLY ONE PROTON DIFFERENCE

28) B) H3O^+

        H^+    +    H2O ---------------------------->    H3O^+

29) B) NH3 AND Cl^-1 because both are accepting proton

36) Kc = [NO2]2/[NO]2[O2]1

45)   B.P OF A SOLUTION IS DIRECTLY PROPOTIONAL TO THE i*m

     answer is B Al(NO3)3 BECAUSE i=4 , Al+3 + 3 NO3-

48) 1/2 RATE OF DISAPPEARENCE OF NO2 = RATE OF APPEARENCE OF O2

RATE OF APPEARENCE OF O2 = (1/2)*((0.0100-0.00650)/100)

RATE OF APPEARENCE OF O2 = 1.75*10^-5

45)

M= (wt.of KOH)/(m,wt of KOH*volume)

    = 350/(56.10*5.75)

   = 1.085M

43) P^H = -log[H^+]

     HNO3---------------------------> H^+     NO3^-1

     0.250M                          0.250       0.250

P^H = -log(0.250)

       = 0.602

44) P^H + P^OH   = 14

     P^H = 14- P^OH = 14-3.75 = 10.25

42) P^OH = -log[OH^-1]

               = -log (3.4*10^-5)

                 = 4.46

    p^H = 14-P^OH = 14-4.46 = 9.53

41)

P^H = -log[H^+]

11.70 = -log[H^+]

[H^+ ]= 1.99*10^-12

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