Question: what are the active materials of a lead acid battery
[{'answer': 'Lead and lead dioxide', 'provenance': [{'wikipedia_id': '201495', 'title': 'Lead–acid battery', 'start_paragraph_id': 78, 'start_character': 212, 'end_paragraph_id': 78, 'end_character': 233, 'bleu_score': 1.0, 'section': 'Section::::Sulfation and desulfation.\n'}]}, {'answer': 'Lead', 'provenance': [{'wikipedia_id': '201495', 'title': 'Lead–acid battery', 'start_paragraph_id': 0, 'start_character': 0, 'end_paragraph_id': 0, 'end_character': 4, 'bleu_score': 1.0, 'section': 'Section::::Abstract.'}]}, {'answer': 'lead dioxide', 'provenance': [{'wikipedia_id': '201495', 'title': 'Lead–acid battery', 'start_paragraph_id': 20, 'start_character': 88, 'end_paragraph_id': 20, 'end_character': 100, 'bleu_score': 1.0, 'section': 'Section::::Electrochemistry.:Charging.\n'}]}, {'answer': 'sulfuric acid', 'provenance': [{'wikipedia_id': '201495', 'title': 'Lead–acid battery', 'start_paragraph_id': 9, 'start_character': 138, 'end_paragraph_id': 9, 'end_character': 151, 'bleu_score': 1.0, 'section': 'Section::::Electrochemistry.:Discharge.\n'}]}, {'provenance': [{'wikipedia_id': '201495', 'title': 'Lead–acid battery', 'start_paragraph_id': 0, 'start_character': 0, 'end_paragraph_id': 0, 'end_character': 0, 'bleu_score': 1.0, 'meta': {'yes_no_answer': 'NONE', 'annotation_id': 15030494417497024014}, 'section': 'Section::::Abstract.'}]}, {'provenance': [{'wikipedia_id': '201495', 'title': 'Lead–acid battery', 'start_paragraph_id': 78, 'start_character': 0, 'end_paragraph_id': 78, 'end_character': 857, 'bleu_score': 0.985238839858627, 'meta': {'yes_no_answer': 'NONE', 'annotation_id': 15030494417497024014}, 'section': 'Section::::Sulfation and desulfation.\n'}]}, {'provenance': [{'wikipedia_id': '201495', 'title': 'Leadacid battery', 'section': 'Section::::Electrochemistry.:Discharge.\n', 'start_paragraph_id': 9, 'end_paragraph_id': 9, 'meta': {'evidence_span': ['In the discharged state both the positive and negative plates become lead(II) sulfate (), and the electrolyte loses much of its dissolved sulfuric acid and becomes primarily water.', 'In the discharged state both the positive and negative plates become lead(II) sulfate (), and the electrolyte loses much of its dissolved sulfuric acid and becomes primarily water.\rhighlight sentence(s) containing evidence, not only the answer', 'In the discharged state both the positive and negative plates become lead(II) sulfate (), and the electrolyte loses much of its dissolved sulfuric acid and becomes primarily water.']}}]}, {'provenance': [{'wikipedia_id': '41382162', 'title': 'Battery regenerator', 'section': 'Section::::Background.\n', 'start_paragraph_id': 4, 'end_paragraph_id': 4, 'meta': {'evidence_span': ['Conventional leadacid batteries consist of a number of plates of lead and lead dioxide suspended in a cell filled with weak sulfuric acid. Lead oxide reacts with the sulfur and oxygen in the acid to give up an electron, leaving the plate positively ch', 'sulfate to flake off the plates and eventually dissolve. Conventional leadacid batteries consist of a number of plates of lead and lead dioxide suspended in a cell filled with weak sulfuric acid. Lead oxide reacts with the sulfur and oxygen in the acid to give up an electron, leaving the plate positively charged and producing lead sulfate. Lead reacts with the acid by taking in two electrons, leaving it negative while also producing lead sulfate. The two chemical processes continue as long as an external circuit is available to allow the electrons to flow back into the positive plates, but reaches equilibrium quickly when the battery is disconnected from the circuit. Each complete reaction produces about 2.11V. A typical 12V battery consists of six individual "cells" wired together in a single box, producing 12.66V when fully charged.', 'Conventional leadacid batteries consist of a number of plates of lead and lead dioxide suspended in a cell filled with weak sulfuric acid.']}}]}]