A laboratory technician reacts powdered aluminum metal with chlorine gas to form a…
CHEMISTRY · Multi-part · A Level · Chemistry · Amount of substance · Amount of substance
Problem
A laboratory technician reacts powdered aluminum metal with chlorine gas to form a chloride compound. In a sealed container, 5.40 g of Al reacts completely with Cl₂ to produce 26.6 g of a single product.
Respond to the following prompts.
(a) Show that only one product is formed and determine its empirical formula.
(b) Calculate the moles of Al that reacted and the moles of Cl₂ consumed, using the data in the prompt.
(c) From the mole amounts in part (b), obtain the simplest whole-number mole ratio of Al to Cl₂ and write the balanced equation for the synthesis reaction.
(d) Using your balanced equation, calculate the theoretical mass of Cl₂ that should have reacted; compare it with the experimental value and discuss one possible source of discrepancy.