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b) The standard enthalpy change of combustion (i.e. the heat change) of sucrose is -5644 kJ mol-¹. Calculate the energy released when one sweet containing 6.70 g of sucrose is completely burnt. c) A man needs to consume about 2500 dietary calories (i.e. 2500 kcal) per day. Given that 1 kJ = 0.239 kcal, how many sweets would a man have to consume in order to meet his daily calorific requirement?

b) The standard enthalpy change of combustion (i.e. the heat change) of sucrose is -5644 kJ mol-¹. Calculate the energy released when one sweet containing 6.70 g of sucrose is completely burnt. c) A man needs to consume about 2500 dietary calories (i.e. 2500 kcal) per day. Given that 1 kJ = 0.239 kcal, how many sweets would a man have to consume in order to meet his daily calorific requirement?

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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b) The standard enthalpy change of combustion (i.e. the heat change) of sucrose is -5644 kJ mol-¹. Calculate the energy released when one sweet containing 6.70 g of sucrose is completely burnt. c) A man needs to consume about 2500 dietary calories (i.e. 2500 kcal) per day. Given that 1 kJ = 0.239 kcal, how many sweets would a man have to consume in order to meet his daily calorific requirement? Sherbet produces a fizzing sensation in the mouth when its two main components, tartaric acid and sodium hydrogencarbonate, react together in aqueous solution to make carbon dioxide gas. The reaction is given below: H₂C₂H4O6 + 2NaHCO3 Sodium Bicarbonate Tartaric Acid Na₂C4H₂O6 + 2H₂O + Sodium Water Tartarate 2CO₂ Carbon Dioxide
Transcribed Image Text:b) The standard enthalpy change of combustion (i.e. the heat change) of sucrose is -5644 kJ mol-¹. Calculate the energy released when one sweet containing 6.70 g of sucrose is completely burnt. c) A man needs to consume about 2500 dietary calories (i.e. 2500 kcal) per day. Given that 1 kJ = 0.239 kcal, how many sweets would a man have to consume in order to meet his daily calorific requirement? Sherbet produces a fizzing sensation in the mouth when its two main components, tartaric acid and sodium hydrogencarbonate, react together in aqueous solution to make carbon dioxide gas. The reaction is given below: H₂C₂H4O6 + 2NaHCO3 Sodium Bicarbonate Tartaric Acid Na₂C4H₂O6 + 2H₂O + Sodium Water Tartarate 2CO₂ Carbon Dioxide
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12:13 2 of 5 D < Question 1 The simplest carboxylic acid is methanoic acid (or formic acid), HCOOH, which occurs naturally in ants. When an ant bites, it injects an aqueous solution of 50% (by volume) methanoic acid, typically injecting around 6.0 × 10-³ mL of this solution. a) For each sting, the ant does not inject all of its methanoic acid but keeps a little in reserve. Assuming that a typical ant injects 80% of its methanoic acid, what is the total volume of pure methanoic acid contained in a 'typical ant'? b) How many 'typical' ants would have to be distilled to produce 1 L of pure methanoic acid? Sodium hydrogencarbonate, NaHCO3, is often used to treat ant stings. The reaction between methanoic acid and sodium hydrogencarbonate is: HCOOH + NaHCO3 → HCOO +Na* + H2O + CO2 c) Given that the density of methanoic acid is 1.2 g mL-¹, how many moles of methanoic acid does a typical ant inject? d) What mass (g) of sodium hydrogencarbonate would be required to completely neutralise a typical ant sting? Question 2 Sherbet lemons are sweets which consist of a flavoured sugar (sucrose, C12H22O11) shell filled with sherbet. The sherbet contains sodium hydrogencarbonate, NaHCO3 and tartaric acid (2,3- dihydroxybutanedioic acid): HO₂C HO H Tartaric acid 384 CO₂H OH H a) Write an equation for the complete combustion of sucrose in excess oxygen, which gives carbon dioxide and water. b) The standard enthalpy change of combustion (i.e. the heat change) of sucrose is -5644 kJ moodlecurrent.gre.ac.uk
Transcribed Image Text:12:13 2 of 5 D < Question 1 The simplest carboxylic acid is methanoic acid (or formic acid), HCOOH, which occurs naturally in ants. When an ant bites, it injects an aqueous solution of 50% (by volume) methanoic acid, typically injecting around 6.0 × 10-³ mL of this solution. a) For each sting, the ant does not inject all of its methanoic acid but keeps a little in reserve. Assuming that a typical ant injects 80% of its methanoic acid, what is the total volume of pure methanoic acid contained in a 'typical ant'? b) How many 'typical' ants would have to be distilled to produce 1 L of pure methanoic acid? Sodium hydrogencarbonate, NaHCO3, is often used to treat ant stings. The reaction between methanoic acid and sodium hydrogencarbonate is: HCOOH + NaHCO3 → HCOO +Na* + H2O + CO2 c) Given that the density of methanoic acid is 1.2 g mL-¹, how many moles of methanoic acid does a typical ant inject? d) What mass (g) of sodium hydrogencarbonate would be required to completely neutralise a typical ant sting? Question 2 Sherbet lemons are sweets which consist of a flavoured sugar (sucrose, C12H22O11) shell filled with sherbet. The sherbet contains sodium hydrogencarbonate, NaHCO3 and tartaric acid (2,3- dihydroxybutanedioic acid): HO₂C HO H Tartaric acid 384 CO₂H OH H a) Write an equation for the complete combustion of sucrose in excess oxygen, which gives carbon dioxide and water. b) The standard enthalpy change of combustion (i.e. the heat change) of sucrose is -5644 kJ moodlecurrent.gre.ac.uk
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