Question 9 (16 marks) In a laboratory, an experiment was carried out to demonstrate the chemical reaction between
nitric acid and sodium hydrogencarbonate. The molecular equation can be written as follows.
I
HNO3(aq) + NaHCO3(s) - NaNO3(aq) + CO2(g) + H2O(1)

Calculate the volume of CO2(g) that is produced at 25 °C and 1.00 atm when 10.0 mL of 2.00
mol/L HNO3 reacts with 1.00 g NaHCO3 (molar mass = 84.006 g/mol). Clearly show your
working, including a statement about the mole ratios of the substances in the reaction, and state
the unit.​

Under what conditions will a gas be most likely to exhibit the ideal gas properties predicted by the ideal gas law? 1)high pressures and high temperature, because particles are forced closer together with higher kinetic energy, so intermolecular forces of attraction are weaker 2)high pressure and low temperature, because particles are forced closer together and moving slower, so the volume of the particles is less significant 3) low pressure and high temperature, because particles are spread farther apart and moving faster, so the intermolecular forces of attraction are weaker 4)low pressure and low temperature, because particles are spread farther apart with lower kinetic energy, so the volume of the particles is less significant