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Question 44

Potassium hydrogencarbonate solution and dilute nitric acid react together to form potassium nitrate, water, and carbon dioxide gas.

The equation for the reaction is:

KHCO3(aq)+HNO3(aq)→KNO3(aq)+H2O(l)+CO2(g) \text{KHCO}_3(\text{aq}) + \text{HNO}_3(\text{aq}) \rightarrow \text{KNO}_3(\text{aq}) + \text{H}_2\text{O}(\text{l}) + \text{CO}_2(\text{g}) KHCO3​(aq)+HNO3​(aq)→KNO3​(aq)+H2​O(l)+CO2​(g)

A student performs an experiment using the following conditions:

  • Concentration of potassium hydrogencarbonate solution = 0.150 mol/dm30.150\text{ mol/dm}^30.150 mol/dm3
  • Volume of potassium hydrogencarbonate solution = 40 cm340\text{ cm}^340 cm3
  • Volume of deionised water = 20 cm320\text{ cm}^320 cm3
  • Volume of dilute nitric acid = 20 cm320\text{ cm}^320 cm3 (the nitric acid is in excess)
a.

Calculate the mass of carbon dioxide, CO2\text{CO}_2CO2​, formed in this experiment. (ArA_rAr​: C=12\text{C} = 12C=12, O=16\text{O} = 16O=16)

[4]
b.

The solubility of carbon dioxide in the final mixture at room temperature is 1.60 g/dm31.60\text{ g/dm}^31.60 g/dm3. Use this information to explain whether any carbon dioxide gas escapes from the flask during the experiment.

[3]

Chemical formulae, equations and calculations Questions

  1. IGCSE
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  3. /Chemical formulae, equations and calculations