INSTRUCTIONS TO CANDIDATES:
- Write your name and index number in the spaces provided above.
- Sign and write the date of examination in the spaces provided above.
- Answer ALL the questions in the spaces provided.
- Mathematical tables and silent electronic calculators may be used.
- All working must be clearly shown where necessary.
- Candidates should check the question paper to ascertain that all the pages are printed as indicated and that no questions are missing
For Examiner’s Use Only
Questions |
Maximum Score |
Candidate’s Score |
1-30 | 80 |
QUESTIONS
- The samples of equal volumes of water were put in 100cm3 conical flasks and heated for 5 minutes on a Bunsen flame. It was observed that sample 1 registered a low temperature than sample II
- Name flame I (1mk)
- State one disadvantage of using flame I for heating (1mk)
- Study the diagram below and answer the questions that follow.
The diagram shows the method used to separate component of mixture P- Name X (1mk)
- What is the name given to the method used in separation of mixture P (½mk)
- What would happen if the inlet and outlet of water were interchanged ( ½mk)
- Which physical property is used to separate mixture P (1mk)
- The table below shows the solubility of three solids P, Q, and R.
SOLID COLD WATER HOT WATER P soluble soluble Q insoluble insoluble R insoluble soluble - State why a water molecule H2O can combine with H+ ion to form H3O+ ion (1mk)
- The PH values of some solutions are given below
PH 14.0 1.0 8.0 6.5 7.0 Solution M L N P Z - Identify the solution with the lowest concentration of hydrogen ion. Give reason for your answer (1mk)
- Which solution would be used as an anti-acid for treating stomach upset. Give for your answer (1mk)
- The data below gives the electronic configuration of some selected atoms and ions
Atom / ion A2+ B C2- D2+ E F- G+ H Electronic configuration 2 2.4 2.8 2.8.8 2.8 2.8.8 0 2.8.2 - Select an atom that is a noble gas (1mk)
- What is the atomic number of C and A (1mk)
- Select an element that belong to group 2 and period four (1mk)
- Write the formula of the compound formed when D and F react (1mk)
- Helium is used instead of hydrogen in balloons for metrological research. Explain (1mk)
- Zinc metal and hydrochloric acid reacts according to the following equation
Zn(s) + 2HCl (aq) → ZnCl2 (aq) + H2 (g)
1.96g of Zinc metal were reacted with 100cm3 of 0.2M hydrochloric acid- Determine the reagent that was in excess (2mks)
Zn=65.2; Molar gas volume at s.t.p 22.4 liters - Calculate the total volume of hydrogen gas that was liberated at s.t.p (1mk)
- Determine the reagent that was in excess (2mks)
- Give the IUPAC names of the following compounds (1mk)
- CH3CH2CH2CH CH3
l
CH3 ……………………………………………………………………………. - CH3CH=CHCl …………………………………………………………………………… (1mk)
- CH3CH2CH2CH CH3
- 0.9g of potassium chloride and potassium carbonate mixture completely reacted with 25cm3 of 0.2M hydrochloric acid
- Write an equation of the reaction which takes place (1mk)
- Determine the number of moles of the acid used (1mk)
- Calculate the mass of potassium chloride in the mixture (K=39.0; C=12.0; O=16.0) (2mks)
- Study the flow chart below and answer the questions that follow
- Identify metal M: ………………………………………………………. (1mk)
- Colourless gas: …………………………………………………………. (1mk)
- Write an equation that leads to the formation of white precipitate in process (1mk)
-
- Define the term dynamic equilibrium (1mk)
- A reaction at equilibrium can be represented as
2CrO2-4[aq] +2H+[aq] ↔ Cr2O7 2-[aq] + H2O{l}
Yellow orange
State and explain the observation made when NaOH is added to the equilibrium mixture (2mks)
- Few drops of hydrochloric acid were added into a test tube containing lead {II} Nitrate solution
- State one observation made (1mk)
- Write an ionic equation of the reaction that occurred in the test tube (1mk)
- A compound of carbon, hydrogen and oxygen contains 57.15% carbon, 4.76% hydrogen and the rest oxy gen. If its relative molecular mass is 126, find its molecular formula. (C = 12, H = 1, O = 16) (3mks)
- Study the information in the table below and answer the questions that follow.
Salt
Solubility g/100g of water
At 40°C
At 60°C
CuSO4
28
38
Pb(NO3)2
79
98
- Which salt crystallized out? Give a reason. (2 marks)
- Calculate the mass of the salt that crystallized out. (1 mark)
-
- Distinguish between strong and concentrated acid ( 1mk)
- A solution of ammonia in methylbenzene has no effects on red litmus paper while a solution of ammonia in water turns red litmus paper blue. Explain (2mks)
- Name the process which takes place when
- Iodine changes directly from solid to gas (1mk)
- Fe2+( aq) changes to Fe3+(aq) (1mk)
- White sugar changes to black when mixed with concentrated sulphuric (VI) acid (1mk)
- In the last stage of the solvay process, a mixture of sodium hydrogen carbonate and ammonium chloride is formed
- State the method of separation used (1mk)
- Write an equation showing how lime is slaked (1mk)
- Name the by- product recycled in the above process (1mk)
- The diagram below is a section of a model of the structure of element K
- State the type of bonding that exist in K (1mk)
- In which group of the periodic table does element K belong. Give a reason (2mks)
- Study the diagram below and answer the questions that follow
- State two observations made in the above experiment when sodium react with water (2 mks)
- Write a chemical equation for the reaction that takes place (1mk)
-
- Explain why permanent hardness in water cannot be removed by boiling (2mks)
- Name two methods that can be used to remove permanent hardness from water (1mk)
- Write an equation to show the effect of heat on the nitrate of: - (2mks)
- Potassium……………………………………………………………………………………………..
- Silver…………………………………………………………………………………………………..
- Study the diagram below and use it to answer the questions that follow.
- State the observation made in the combustion tube. (1mk)
- Write an equation for the reaction that took place in the combustion tube. (1mk)
- Name gas P (1mk)
- Sulphur exists in two crystalline forms.
- Name one crystalline form of Sulphur. (1mk)
- State two uses of Sulphur. (2mks)
- Bond energies for some bonds are tabulated below: -
BOND
BOND ENERGY KJ/mol
H – H
436
C = C
610
C- H
410
C – C
345
C2H4 (g) + H2(g) → C2H6(g) - Study the set up below and answer the questions that flows
State all the observations that would be made when the circuit is completed (3mks) - Describe how solid samples of salts can be obtained from a mixture of lead (II) chloride, sodium chloride and ammonium chloride. (3mks)
- The diagram below represents a set-up used to prepare oxygen gas.
- Name substance Q. (1mk)
- Complete the set-up to show how oxygen gas is collected. (1mk)
- Write the equation for the reaction that occur. (1mk)
- Two reagents that can be used to prepare chlorine gas are potassium manganate (VII) and hydrochloric acid.
- Write an equation for the reaction. (1mk)
- Give the formula of another reagent that can be used instead of potassium manganate (VII). (1mk)
- Using an equation illustrate how chlorine bleach coloured substances. (2mks)
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