Question 1:
Diagram 1 shows the setting up of apparatus in an experiment.
(a) Name the process in Diagram 1. [1 mark]



(b)(i) Name metal Q. [1 mark]
 
(ii) What happens to metal Q during the process in Diagram 1? [1 mark]

(c) Which metal functions as the cathode? [1 mark]

(d)(i) What will happen to the iron key at the end of the experiment? [1 mark]
 
(ii) State one method to get a good result in (d)(i) [1 mark]


Answer:
(a) Electroplating

(b)(i) Copper
(b)(ii) Metal Q dissolves in the copper(II) sulphate solution to form copper ions and becomes thinner.

(c) Iron key.

(d)(i) The surface of the iron key will be coated with a brown layer of copper.
(d)(ii) The surface of the metal to be plated must be cleaned with sandpaper before electrolysis begins.

Question 1:
Diagram below shows the extraction of tin ore at high temperature in a blast furnace.


(a) Name two elements in R. [2 marks]

(b) State one reason why carbon is a suitable element to use in the extraction of tin ore from R? [1 mark]

(c) Name gas S. [1 mark]

(d) What is the function of limestone in this process? [1 mark]

(e) Name product T. [1 mark]


Answer:
(a) Tin, oxygen

(b) As tin is less reactive than carbon, carbon can be used to reduce the tin ore from R.

(c) Carbon dioxide.

(d) The limestone is decomposed to produce quicklime (calcium oxide) which combines with impurities such as silica to form slag.

(e) Slag
 

Question 1:
Diagram 1.1 and Diagram 1.2 show an experiment to study the reactivity of metals with water.



(a) Observe Diagram 1.1. State the volume of gas collected.
  Write down your answer in Table below. [1 mark]


(b) Based on the result in Table above, state one inference. [1 mark]

(c) State the variables in this experiment.
(i) Constant variable [1 mark]
(ii) Responding variable [1 mark]

(d) Based on this experiment, mark (\/) the metal which is more reactive. [1 mark]
$\begin{array}{l}\text{Sodium }\boxed{}\\ \text{Calcium }\boxed{}\end{array}$


Answer:
(a)

(b) A reactive metal can displace more gas from water.

(c)(i) The mass of the metal / The time taken

(c)(ii) The volume of gas collected

(d)
$\begin{array}{l}\text{Sodium }\boxed{\vee }\\ \text{Calcium }\boxed{}\end{array}$

Question 1:
Diagram 1.1 and Diagram 1.2 show an experiment to study the heat change in chemical reactions at room temperature.



(a) Based on Diagram 1.1, what is your observation about the change in temperature?
  Mark (\/) for your answer in Table below. [1 mark]


(b) What is the final reading for the thermometer in Diagram 1.2? [1 mark]

(c) State the variables in this experiment.
(i) Constant variable [1 mark]
(ii) Responding variable [1 mark]

(d) State one hypothesis for this experiment. [1 mark]


Answer:
(a)

(b) 35 ^oC

(c)(i) The amount of water or initial temperature

(c)(ii) The final temperature

(d) In a chemical reaction, heat is given out causing a rise in temperature or is absorbed causing a drop in temperature.