Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Unit
Physical Chemistry
442 practice questions
Topics covered
Practice questions
181–190 of 442
Question 181
3 marks · Easy
Answer and see the solution →In an experiment, 0.40 g of carbon dioxide is produced in the first 50 seconds during a reaction between calcium carbonate and hydrochloric acid.
(a)[1 mark]Write down the formula for calculating the average rate of reaction.
(b)[2 marks]Calculate the average rate of reaction in g/s.
Question 182
2 marks · Easy
Answer and see the solution →A student plots a graph showing the initial rate of reaction versus concentration of a reactant. At 0.80 mol/dm³, the rate is 0.011 g/s. Predict the rate if the concentration is increased to 1.60 mol/dm³, assuming the rate is directly proportional to concentration.
Question 183
2 marks · Normal
Answer and see the solution →Describe what happens to the rate of a chemical reaction when the concentration of one of the reactants is increased. Explain your answer.
Question 184
4 marks · Normal
Answer and see the solution →A student is given a bottle of 2.00 mol/dm³ hydrochloric acid. She prepares diluted solutions for a reaction experiment. The total final volume of each solution will be 25.0 cm³.
(a)[2 marks]Calculate the concentration (in mol/dm³) if she mixes 8.0 cm³ of the original acid with 17.0 cm³ of distilled water.
(b)[2 marks]Calculate the concentration (in mol/dm³) if she instead uses 20.0 cm³ of the original acid and 5.0 cm³ of water, making the total volume up to 25.0 cm³.
Question 185
3 marks · Normal
Answer and see the solution →In an experiment, a student finds that 0.21 g of carbon dioxide are released in the first 30 seconds of a reaction between marble chips and hydrochloric acid. Calculate the average rate of reaction (in g/s) during this time. Show your working.
Question 186
3 marks · Normal
Answer and see the solution →Explain how you can tell from a graph whether the rate of reaction is directly proportional to the concentration of the reactant.
Question 187
4 marks · Normal
Answer and see the solution →The table below gives the concentration of a reactant and the corresponding average rate of reaction measured at the start of an experiment.
Concentration of reactant and average rate Concentration of HCl (mol/dm³) Average rate (g/s) 0.50 0.004 1.00 0.008 1.50 0.012 2.00 0.016 (a)[1 mark]Describe the pattern shown by the data.
(b)[1 mark]Predict the average rate if the concentration is increased to 2.50 mol/dm³.
(c)[2 marks]Explain your answer to part b.
Question 188
1 mark · Normal
Answer and check →Which of the following is the concentration (in mol/dm³) of a solution made by mixing 6.0 cm³ of 2.00 mol/dm³ hydrochloric acid with 19.0 cm³ of distilled water to make a total of 25.0 cm³?
- A.0.30 mol/dm³
- B.0.40 mol/dm³
- C.0.48 mol/dm³
- D.0.60 mol/dm³
Question 189
2 marks · Normal
Answer and see the solution →A reaction between powdered magnesium and dilute hydrochloric acid releases 0.30 g of hydrogen in the first 20 seconds. Calculate the average rate of production of hydrogen gas in g/s.
Question 190
4 marks · Normal
Answer and see the solution →Look at the following graph, which shows the rate of reaction (y-axis, in g/s) against concentration of hydrochloric acid (x-axis, in mol/dm³) for a certain reaction.
Rate of reaction vs concentration of HCl (a)[1 mark]Describe the shape and position of the line on the graph.
(b)[1 mark]What does this show about the relationship between the concentration of hydrochloric acid and the rate of reaction?
(c)[2 marks]If the concentration is doubled, what happens to the rate of reaction? Explain your answer.