Date | May 2011 | Marks available | 1 | Reference code | 11M.1.sl.TZ1.14 |
Level | SL | Paper | 1 | Time zone | TZ1 |
Command term | Solve | Question number | 14 | Adapted from | N/A |
Question
When \({\text{100 c}}{{\text{m}}^{\text{3}}}\) of \({\text{1.0 mol}}\,{\text{d}}{{\text{m}}^{ - 3}}\) HCl is mixed with \({\text{100 c}}{{\text{m}}^{\text{3}}}\) of \({\text{1.0 mol}}\,{\text{d}}{{\text{m}}^{ - 3}}\) NaOH, the temperature of the resulting solution increases by 5.0 °C. What will be the temperature change, in °C, when \({\text{50 c}}{{\text{m}}^{\text{3}}}\) of these two solutions are mixed?
A. 2.5
B. 5.0
C. 10
D. 20
Markscheme
B
Examiners report
There were three G2 comments on this question. Some suggested that it would be better if more consistent use of significant figures would be used, which is noted and one stated that the question was complicated. The question was certainly challenging for candidates and only 36.27% of candidates got the correct answer B.
Syllabus sections
- 17N.2.sl.TZ0.2b: Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group.
- 17N.2.sl.TZ0.1d.ii: Calculate the enthalpy change, ΔH, in kJ mol–1, for the reaction between ethanoic acid and...
- 17N.2.sl.TZ0.1d.i: Determine the heat change, q, in kJ, for the neutralization reaction between ethanoic acid...
- 17N.1.sl.TZ0.13: Which statement is correct for this reaction? Fe2O3 (s) + 3CO (g) → 2Fe (s) + 3CO2 (g) ...
- 17N.2.hl.TZ0.3b: Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group...
- 17N.1.hl.TZ0.19: The enthalpy change for the dissolution of NH4NO3 is +26 kJ mol–1 at 25 °C. Which statement...
- 17N.1.hl.TZ0.17: The combustion of glucose is exothermic and occurs according to the following...
- 17M.2.hl.TZ2.8b.v: State a technique other than a pH titration that can be used to detect the equivalence point.
- 17M.2.sl.TZ2.8a.ii: The energy released by the reaction of one mole of hydrogen peroxide with hydroquinone is...
- 17M.3.sl.TZ1.15c: Explain, in terms of the molecular structure, the critical difference in properties...
- 17M.3.sl.TZ1.5f: Outline why the thermochemical method would not be appropriate for 0.001...
- 17M.3.sl.TZ1.5d: State one other assumption that is usually made in the calculation of the heat produced.
- 17M.3.sl.TZ1.5c: Suggest how heat loss could be reduced.
- 17M.3.sl.TZ1.5b: Heat losses would make this method less accurate than the pH probe method. Outline why the...
- 17M.3.sl.TZ1.5a: Explain how the concentration may be calculated in this way.
- 17M.2.sl.TZ1.4f: Determine the enthalpy change of reaction, ΔH, in kJ, when 1.00 mol of gaseous hydrazine...
- 17M.2.sl.TZ1.4e: Hydrazine has been used as a rocket fuel. The propulsion reaction occurs in several stages...
- 17M.1.sl.TZ1.13: Which expression gives the mass, in g, of ethanol required to produce 683.5 kJ of heat...
- 16N.1.sl.TZ0.15: 5.35g of solid ammonium chloride, NH4Cl(s), was added to water to form 25.0g of solution. The...
- 16N.1.sl.TZ0.1: Which change of state is exothermic? A. CO2(s) → CO2(g)B. H2O(l) → H2O(g) C. NH3(g) →...
- 16M.3.sl.TZ0.10b: Calculate the energy, in kJ, produced from 15.0g of glucose if its enthalpy of combustion is...
- 16M.2.hl.TZ0.1d: Impurities cause phosphine to ignite spontaneously in air to form an oxide of phosphorus and...
- 16M.2.sl.TZ0.2a: (i) 200.0 g of air was heated by the energy from the complete combustion of 1.00 mol...
- 16M.1.sl.TZ0.13: When 25.0cm3 0.100moldm−3 NaOH(aq) is mixed with 25.0cm3 0.100moldm−3 HCl(aq) at the same...
- 15M.1.hl.TZ1.14: The same amount of heat energy is added to 1.00 g of each substance. Which statement is...
- 15M.1.hl.TZ1.16: Which equation represents the standard enthalpy of formation of liquid methanol? A. ...
- 15M.1.hl.TZ2.16: Which equation represents the standard enthalpy change of formation, \(\Delta H_f^\Theta \),...
- 15M.2.hl.TZ2.3a: Calculate the standard enthalpy change, \(\Delta {H^\Theta }\), in...
- 15M.1.sl.TZ1.14: Which processes are exothermic? I. ...
- 15M.1.sl.TZ2.14: Which combination is correct for the standard enthalpy change of neutralization?
- 15M.2.sl.TZ1.5b.iv: Explain why the reaction is exothermic in terms of the bonds involved.
- 14M.1.sl.TZ1.14: Which statement is correct for the reaction with this enthalpy level diagram? A. Heat...
- 14M.1.sl.TZ1.15: The specific heat capacities of two substances are given in the table below. Which...
- 14M.1.sl.TZ2.14: The table shows information about temperature increases when an acid and an alkali are...
- 14M.1.sl.TZ2.16: What is the temperature rise when 2100 J of energy is supplied to 100 g of water? (Specific...
- 14M.1.sl.TZ2.15: What is the value of \(\Delta H\) for the exothermic reaction represented by the diagram...
- 14M.2.sl.TZ2.6g.iv: The standard enthalpy change of combustion of A is...
- 14M.3.sl.TZ1.5a: When 1.13 g of a granola bar was combusted in a bomb calorimeter, the temperature of...
- 14N.2.hl.TZ0.2b: (i) Define the term standard enthalpy change of formation. (ii) ...
- 14N.2.hl.TZ0.11e: Hydrochloric acid neutralizes sodium hydroxide, forming sodium chloride and...
- 14N.1.sl.TZ0.14: The enthalpy change for the reaction between zinc metal and copper(II) sulfate solution is...
- 14N.2.sl.TZ0.7e: (i) Define the term standard enthalpy change of reaction, \(\Delta {H^\Theta...
- 13N.1.hl.TZ0.15: Which processes are exothermic? I. ...
- 13N.1.hl.TZ0.17: Which ionic compound has the most endothermic lattice enthalpy? A. Sodium chloride B. ...
- 13N.2.sl.TZ0.4g.ii: Explain how the results of this experiment could be used to calculate the molar enthalpy...
- 13N.1.sl.TZ0.15: Which processes are exothermic? I. ...
- 13N.2.sl.TZ0.4g.i: Methanol can also be burnt as a fuel. Describe an experiment that would allow the molar...
- 13M.1.hl.TZ1.15: Which process is endothermic? A. ...
- 13M.2.sl.TZ1.7a.i: Calculate the enthalpy change of combustion of methanol.
- 13M.2.sl.TZ1.7a.ii: Using the theoretical value in Table 12 of the Data Booklet, discuss the experimental...
- 13M.1.hl.TZ2.16: Which reaction has an enthalpy change equal to the standard enthalpy change of...
- 13M.2.hl.TZ2.5a.iii: Define the term standard enthalpy change of formation, \(\Delta H_{\text{f}}^\Theta \).
- 13M.2.hl.TZ2.5a.iv: Calculate the standard enthalpy change for the reaction, \(\Delta {H^\Theta }\), in...
- 13M.1.sl.TZ2.15: Which statements are correct for an exothermic reaction? I. The products are more stable...
- 13M.1.sl.TZ2.16: The specific heat capacity of aluminium is...
- 13M.2.sl.TZ2.6c.iii: State whether the reaction given in stage 1 is exothermic or endothermic.
- 12N.1.sl.TZ0.14: Which combination is correct for the exothermic reaction that occurs between zinc and copper...
- 12N.1.sl.TZ0.15: A 5.00 g sample of a substance was heated from 25.0 °C to 35.0 °C using...
- 12N.2.sl.TZ0.1a: (i) State the number of significant figures for the masses of...
- 10N.2.hl.TZ0.7c: (i) The enthalpy change of formation, \(\Delta H_{\text{f}}^\Theta \), of liquid...
- 10N.1.sl.TZ0.14: Which statement is correct given the enthalpy level diagram below? A. The reaction is...
- 10N.1.sl.TZ0.15: Identical pieces of magnesium are added to two beakers, A and B, containing hydrochloric...
- 09N.2.hl.TZ0.7b.i: The standard enthalpy change of three combustion reactions is given below in...
- 09N.2.hl.TZ0.7b.v: Suggest with a reason, why the values obtained in parts (b) (i) and (b) (iv) are different.
- 09N.1.sl.TZ0.16: In a reaction that occurs in 50 g of aqueous solution, the temperature of the reaction...
- 09N.1.sl.TZ0.15: Which is true for a chemical reaction in which the products have a higher enthalpy than the...
- 10M.2.sl.TZ1.6a: (i) Use the data to calculate the heat evolved when the ethanol was combusted. (ii) ...
- 10M.1.sl.TZ2.16: Which is correct about energy changes during bond breaking and bond formation?
- 10M.1.sl.TZ2.17: Which processes are exothermic? I. Ice melting II. Neutralization III. ...
- 09M.1.hl.TZ1.14: 1.0 g of sodium hydroxide, NaOH, was added to 99.0 g of water. The temperature of the...
- 09M.2.hl.TZ1.6b.ii: Deduce which two of the enthalpy changes a to e have negative signs.
- 09M.1.sl.TZ1.15: When some solid barium hydroxide and solid ammonium thiosulfate were reacted together, the...
- 09M.1.sl.TZ1.17: Some water is heated using the heat produced by the combustion of magnesium metal. Which...
- 09M.1.sl.TZ2.14: What is the energy, in kJ, released when 1.00 mol of carbon monoxide is burned according to...
- 09M.2.sl.TZ2.6a.iii: The standard enthalpy change for the complete combustion of octane,...
- 09M.1.sl.TZ2.16: Which of the following reactions are exothermic? I. ...
- 09M.1.sl.TZ2.15: The specific heat of iron is \({\text{0.450 J}}\,{{\text{g}}^{ - 1}}{{\text{K}}^{ - 1}}\)....
- 11M.2.sl.TZ1.1b.ii: Calculate the heat absorbed, in kJ, by the water.
- 11M.2.sl.TZ1.1c.ii: Part (b)
- 11M.2.sl.TZ1.4a.ii: Calculate the amount, in mol, of ethanol and octane in 1.00 kg of the fuel mixture.
- 11M.2.sl.TZ1.4a.iii: Calculate the total amount of energy, in kJ, released when 1.00 kg of the fuel mixture is...
- 11M.2.sl.TZ1.1b.iii: Determine the enthalpy change, in \({\text{kJ}}\,{\text{mo}}{{\text{l}}^{ - 1}}\), for the...
- 11M.2.hl.TZ2.6b.i: Outline why the value for the standard enthalpy change of formation of hydrogen is zero.
- 11M.2.hl.TZ2.6b.ii: Calculate the standard enthalpy change for the hydrogenation of propene.
- 11M.1.sl.TZ2.15: Which processes have a negative enthalpy change? I. ...
- 11M.2.sl.TZ2.1a.iv: Determine the value of \(\Delta {H_1}{\text{ in kJ}}\,{\text{mo}}{{\text{l}}^{ - 1}}\).
- 11M.1.sl.TZ2.17: At 25 °C, \({\text{200 c}}{{\text{m}}^{\text{3}}}\) of...
- 11M.2.sl.TZ2.1a.ii: Determine what the temperature rise would have been, in °C, if no heat had been lost to the...
- 11M.2.sl.TZ2.1a.iii: Calculate the heat change, in kJ, when 3.99 g of anhydrous copper(II) sulfate is dissolved in...
- 11M.2.sl.TZ2.1b.ii: Determine the value of \(\Delta {H_2}\) in \({\text{kJ}}\,{\text{mo}}{{\text{l}}^{ - 1}}\).
- 11M.2.sl.TZ2.6a.iv: The value of \({K_{\text{c}}}\) at 500 K is 160 and the value of \({K_{\text{c}}}\) at 700 K...
- 12M.1.sl.TZ2.15: A simple calorimeter was set up to determine the enthalpy change occurring when one mole of...
- 12M.2.sl.TZ2.6d: (i) Sketch and label an enthalpy level diagram for this reaction. (ii) Deduce...
- 11N.2.hl.TZ0.5b.i: Suggest why the \(\Delta H_{\text{f}}^\Theta \) values for...
- 11N.2.hl.TZ0.5b.ii: Determine the standard enthalpy change at 298 K for the reaction.
- 11N.1.sl.TZ0.15: Which process is endothermic? A. ...
- 11N.2.sl.TZ0.6d.i: Define the term endothermic reaction.