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The document outlines experiments investigating the reaction rate of zinc with dilute hydrochloric acid, detailing various conditions and results. It includes questions related to reaction variables, rate definitions, and the effects of catalysts and temperature on equilibrium. Additionally, it discusses the decomposition of dinitrogen tetraoxide and its equilibrium behavior under changing conditions.

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11 views2 pages

Scan 20250416

The document outlines experiments investigating the reaction rate of zinc with dilute hydrochloric acid, detailing various conditions and results. It includes questions related to reaction variables, rate definitions, and the effects of catalysts and temperature on equilibrium. Additionally, it discusses the decomposition of dinitrogen tetraoxide and its equilibrium behavior under changing conditions.

Uploaded by

cebothusi70
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
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DBE/November 2018 Physical Sciences/P2 10 NSC QUESTION 5 (Start on a new Page.) he Feaction of zine and EXCESS dilute hydrochloric acid is used to investigate factors that affect reaction rate. The balanced equation fr he reaction is Zn(s) + 2HCt(aq) —+ ZnCt(aq) + He(9) The reaction conditions used and the results obtained for each experiment are Summarised in the table below. The same mass of zinc is used in all the experiments, The zinc is completely govered reaction time is the time it takes the reaction to be comple! in all reactions, The ‘STATE OF | teMPERATURE | REACTION CONCENTRATION | VOLUME OF JON m TIME (min.) EXPERIMENT | 62! HCE (mokdm?) | He (em) Ona. OF HCe (°C) « 4 ia 2,0 200 powder 25 a 2 7.5 200 granules 25 3 5.0 200 powder 25 s 4 18 400 ‘granules 25 x 5 2.0 200 powder 35 4 5.4 Experiment 1 and experiment 5 are compared. Write down the independent “ variable, 5.2 Define reaction rate. (2) 5.3 White down the value of x in experiment 4. (2) 5.4 The Maxwell-Boltzmann energy distribution curves for particles in each of experiments 1, 3 and § are shown below. ~ Dumber of molecules jE kinetic energy | Identify the graph (Aor Bor °) that represents the following: 5.4.1 Experiment 3 | Give a reason for the answer. (2) 5.42 Experiment § | Give a reason for the answer. (2) Please turn over wight reserved PETE ET RAE Physical Sciences/p2 Hu 5 : . poarion 5 Experiment 6 is now conductod using a catalyst and the CAME Conditions as for Experiment 4 5.6.1 What is the function of the catalyst in this exparinent” ares We that 5.5.2 How will the hoat of roaction in exporinnent 6 wort iy 9 experiment 1? Choose from GREATER THAN, F4 LESS THAN 56 pnpott to 7 Calculate the average rate of the reaction (in mot rnin |) vathy 1° for experiment 2 if 1,5 g of zinc is used QUESTION 6 (Start on a now page.) Dinitrogen tetraoxide, N04(g), decomposes to nitrogen dioxide, NOY). 1 9 © syringe of volume 2 dm® OTC The—mixture reaches equilibrium at 326°C according to the following balanced equation: N2O4(g) = 2NOz (g) colourless brown When equilibrium is reached, it is observed that the colour of the gas in the syringe is brown 61 State Le Chatelier's principle. 62 The syringe is now dipped into a beaker of ice water. After a while the brown colour disappears. the forward reaction EXOTHERMIC or ENDOTHERMIC? i Sener using Le Chatelier's principle, Explain the { 63 The volume of the syringe is now decreased While the te mperature is kept constant. figs will EACH of the following be affe How Wil Ges or REMAINS THE SAME, <1e67 Choose trom: INCREASES, DECRI 63.1 632 The value of the equilibrium constant ‘The number of moles of N,O4(g) a3 Therate ofthe foward and reverse Feactions N2O4(g) wy moles of N2O%(9) were Placed rium Was TEAChid it wae found ye rain 6 of voly a f the 64 Initially X ar 20% of th When equi! ime 3. decomposed @) tad 20, ifthe equitirium ne?" “0 haa value of % a Ii gy NK for he reaction 0, 5 Calculate the ion is 116 at 32 C, cal copytigh" ‘ny Il (A) 6) (2) (3) (4) (4) (1) (8) Me

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