f325.1

1. 1rate=

   1. Aproducts-reactants/ time
   2. Bchange in conc of reactants or products/ change in time
   3. Cchange in conc of reactants or products/ time takes for change to take place
2. 2if the conc of reactants decreases

   1. Afewer collisions take place
   2. Bequilibrium to lhs
   3. Cthe rate slows down
3. 3how to measure a visual change

   1. Aform of a precipitate
   2. Ba colour changge
   3. Cph meter
   4. Dtitration
4. 4how to measure rate of reaction of an acid or a base

   1. Atitration
   2. Bchanges in volume
   3. Cchanges in concerntration
   4. Dph meter
5. 5how to measure reaction rate of a gas

   1. Atitration
   2. Bchanges in volume or pressure
   3. Ca colour change
   4. Dloss of mass of reactants
6. 6zero order

   1. Adirectly affects the rate
   2. Bhas no affect
   3. Caffects the rate squared
7. 7first order ...

   1. Adirectly affects rate
   2. Bhas no affect
   3. Caffects the rate squared
8. 8second order..

   1. Adirectly affects
   2. Bno affect
   3. Caffects the rate squared
9. 9rate equation=

   1. Aa(A)x b(B)
   2. Bk a (A)x b(B)
10. 10rate constant =

    1. Arate / reactants
    2. Breactants/ rate

11. 11a fast reaction has a

    1. Asmall value of k
    2. Ba large value of k
12. 12a slow reaction has a

    1. Asmall value of k
    2. Ba large value of k
13. 13If the rate of reaction [blank_start]increases[blank_end] the rate of reaction [blank_start]increase[blank_end] by [blank_start]increasing[blank_end] the value of k

    1. Aincreases
    2. Bdecerases
    3. Cremains same
    4. Dincrease
    5. Edecrease
    6. Fincreasing
    7. Gdecreasing
14. 14if a reactant appears in the rate equation

    1. Ait is not involved in the rate determining step
    2. Bit is involved in the rate determining step
15. 15an intermediate is

    1. Ainvolved in the over all equation
    2. Bis not in the over all equation
16. 16does the equlibrium law(kc) state that it is reactants/ products

    1. ATrue
    2. BFalse
17. 17if kc<1

    1. Aproduct favoured
    2. Breactant favoured
18. 18if kc>1

    1. Aproduct favoured
    2. Breactant favoured
19. 19if forward reaction s endothermic and the tempreture increases, Kc increases and the products decrease

    1. ATrue
    2. BFalse
20. 20if the forward reaction is exothermic and the tempreture increases, kc increases and the reactants increase

    1. ATrue
    2. BFalse
21. 21if there in a chnage in conc

    1. Akc is changed and equlibrium stays the same
    2. Bkc is the same and equlib is changed
22. 22if the pressure is chnaged

    1. Akc is the same and so is the equilib
    2. Bkc is the same and the equlib changed
    3. Ckc changed and equilb changed
23. 23change in tempreture

    1. Achanges kc and equlib
    2. Bchanges kc and not equilib
24. 24if a compund is (aq) it

    1. Aproduces ions
    2. Bis insoluble
25. 25monobasic acid donate [blank_start]one[blank_end] proton. A tribasic acid produces [blank_start]3[blank_end] protons and dibasic acid produces [blank_start]2[blank_end] protons.

    1. Aone
    2. B2
    3. C3
    4. D3
    5. E1
    6. F2
    7. G2
    8. H3
    9. I1
26. 26conjugate base pairs differ by a

    1. AH+
    2. BOH-
27. 27A STRONG ACID

    1. Apartially dissociates in solution
    2. Bfully dissociates in solution
28. 28a weak acid

    1. Adoes not dissociate in solution
    2. Bpartially disscoiates
29. 29large ka shows

    1. Astonger weak acid
    2. Bweaker weak acid
30. 30small ka means

    1. Aweaker weak acid with small disscoation
    2. Bstronger weak acid with more dissociation
    3. Cweaker weak acid with loads of dissocation
31. 31buffer solutionis amade up of

    1. Aas strong acid
    2. Bconjugate base
    3. Cconjugate acid
    4. Da weak acid
32. 32one method to make a buffer is

    1. Aweak acid
    2. Bsalt of strong acid
    3. Csalt of weak acid
    4. Dsalt of alkali
33. 33one method to make a buffer solution is

    1. Aweak acid
    2. Bstrong acid
    3. Csalt of alkali
    4. Dsalt of weak acid
34. 34another method is

    1. Astrong acid
    2. Bweak acid
    3. Caquesous alkali
    4. Daquesous acid
    5. Enetralisation
35. 35a buffer [blank_start]minimises[blank_end] a PH chnage

    1. Aminimises
    2. Bmaximises
36. 36The addition oh H+ to a [blank_start]buffer[blank_end] solution, increases [H+(aq)]. [blank_start]Conjugate[blank_end] base A- reacts with H+. This causes [blank_start]eqilibrium[blank_end] to shift to the [blank_start]left.[blank_end]

    1. Abuffer
    2. Bacid
    3. Calkali
    4. DConjugate
    5. Epoop
    6. Fleft.
    7. Gright
    8. Heqilibrium
    9. Ireaction
37. 37Addition of [blank_start]oh-[blank_end] to a [blank_start]buffer[blank_end] solution. Causes small amounts of H+ ions to react with oh- ions. HA [blank_start]dissociates[blank_end] to restore H+ ions. Equilibium shifts to the [blank_start]right[blank_end] hand side.

    1. Aoh-
    2. Bright
    3. Cdissociates
    4. Dbuffer
38. 38[blank_start]SA[blank_end][blank_start]WA[blank_end][blank_start]MO[blank_end]

    1. ASA
    2. BSTRONG ACID
    3. CWA
    4. DWEAK ACID
    5. EMO
    6. FMETHYL ORANGE
39. 39 [blank_start]WA[blank_end][blank_start]SA[blank_end][blank_start]P[blank_end]

    1. AWA
    2. BWEKA ACID
    3. CSA
    4. DSTRONG AICD
    5. EP
    6. FPHENYLPHLINE
40. 40wHEN A BASE IS ADDED pH [blank_start]INCREASES[blank_end] SLIGHTLY. tHE Ph the increases [blank_start]quickly[blank_end]. Then when the base is added more there is [blank_start]little[blank_end] chnage in ph

    1. AINCREASES
    2. BDECREASES
    3. Cquickly
    4. DSLOWLY
    5. Elittle
    6. FLARGE
41. 41FOR A STRONG ACID AND STRONG BASE WHAT IS A GOOD INDICATOR

    1. APHENYLPHALINE
    2. BMETHYL ORANGE
42. 42FOR A STRONG ACID AND WEAK BASE..

    1. AP
    2. BMO
43. 43WEAK ACID AND A STRONG BASE

    1. AP
    2. BMO

Description

Singapore-Cambridge GCE Advanced Level(A- Level) Chemistry (f325) Quiz on f325.1, created by Michelle Lewis on 28/03/2016.

Author

Michelle Lewis

Language

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