Chemistry, 17.10.2020 04:01 jjjjjjgegi3088

on plonge une lame de zinc de masse m=2g dans une solution d'acide chlorhydrique (H+aqueux +cl- aqueux) en excès. au cours de la réaction il y a des formations des ions Zn2+ et production d'un gaz qui donne une donation presence d'une flamme. 1) Ecrire les demi équation redox et l'équation bilan entre l'acide chlorhydrique et le zinc. 2)dresser le tableau d'avancement de la réaction et déterminer l'avancement maximal. 3)calculer le volume de d'hydrogène libéré à la fin de la réaction. 4)calculer la masse m du chlorure de zinc formé à la fin de la réaction. on donne Vm=25 L. mol-1 / M (Zn) =64,5 g. mol-1 / M (Cl) =35.5 g. mol-1

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