barometric pressure 101 kpa. Is my working out correct? can you please solve this. Thankyou.
Well done! You have solved the first three problems accurately. I have checked them thoroughly.
(iv) The no. of moles of H2O2 = 4.2*10-3 mol
The final volume = 5+5 = 10 mL = 10*10-3 L
Therefore, the concentration of H2O2 used in the reaction = 4.2*10-3 mol/10*10-3 L
= 0.42 mol/L or 0.42 M
v) The molar mass of H2O2 = 34 g/mol
Therefore, the mass of H2O2 in the original 5 mL sample = 4.2*10-3 mol * 34 g/mol = 0.143 g
vi) The density of H2O2 = 1.45 g/mL
Therefore, the volume of H2O2 in the original 5 mL sample = 0.143 g/(1.45 g/mL) ~ 0.1 mL
vii) The % volume of H2O2 in the total 5 mL sample = (0.1 mL/5 mL) * 100 = 2%
barometric pressure 101 kpa. Is my working out correct? can you please solve this. Thankyou. Trial...
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