text: Question
  
  # In the following reaction, how many grams of hydrogen, H2, will be produced from 53.5 g...
  
  In the following reaction, how many grams of hydrogen, H2, will be produced from 53.5 g of aluminum, Al? 2Al + 3H2SO4 -> 3H2 + Al2(SO4)3
  
  In the following reaction, how many grams of hydrogen, H2, will be produced from 53.5 g of aluminum, Al?
  
  2Al + 3H2SO4 -> 3H2 + Al2(SO4)3
  
  From equation, from 2moles of Al we will get 3moles of H2.
  
  First convert 53.5 g of Al into moles.
  
  Al M.Wt = 27
  
  Al moles = Wt/M.Wt = 53.5/27 = 1.98 moles
  
  So, If 2 moles of Al generates 3 mloles of H2
  
  Then, from 1.98 moles of Al how H2 will produce
  
  =(1.98*3)/2 = 2.972 moles of H2 will produce
  
  Convert 2.972 moles into grams
  
  Moles = wt/m.wt
  
  H2 m.wt = 2
  
  Wt of H2 = 2.972*2 = 5.944 grams of H2 will generate
explanation: The document contains a chemistry problem that involves a stoichiometric calculation. It presents a question about how many grams of hydrogen (H2) will be produced from a given amount of aluminum (Al) in a chemical reaction. The document also provides a detailed step-by-step solution to the problem, including the conversion of grams of aluminum to moles, the use of the stoichiometric ratio from the balanced equation, and the final conversion of moles of hydrogen to grams.
distilabel_metadata.content: Evaluate the user given text extract and determine if it contains a math question and optionally and answer to this question.
  
  Output rules:
  
  1. Briefly describe the document and mention if it contains a question or a question and answer.
  2. Finalize the output with: Label: no-question,question,question-and-answer,multiple-question,multiple-question-and-answer
distilabel_metadata.role: system
distilabel_metadata.content: Question
  
  # In the following reaction, how many grams of hydrogen, H2, will be produced from 53.5 g...
  
  In the following reaction, how many grams of hydrogen, H2, will be produced from 53.5 g of aluminum, Al? 2Al + 3H2SO4 -> 3H2 + Al2(SO4)3
  
  In the following reaction, how many grams of hydrogen, H2, will be produced from 53.5 g of aluminum, Al?
  
  2Al + 3H2SO4 -> 3H2 + Al2(SO4)3
  
  From equation, from 2moles of Al we will get 3moles of H2.
  
  First convert 53.5 g of Al into moles.
  
  Al M.Wt = 27
  
  Al moles = Wt/M.Wt = 53.5/27 = 1.98 moles
  
  So, If 2 moles of Al generates 3 mloles of H2
  
  Then, from 1.98 moles of Al how H2 will produce
  
  =(1.98*3)/2 = 2.972 moles of H2 will produce
  
  Convert 2.972 moles into grams
  
  Moles = wt/m.wt
  
  H2 m.wt = 2
  
  Wt of H2 = 2.972*2 = 5.944 grams of H2 will generate
distilabel_metadata.role: user
distilabel_metadata.raw_output_q_a_detector_0: The document contains a chemistry problem that involves a stoichiometric calculation. It presents a question about how many grams of hydrogen (H2) will be produced from a given amount of aluminum (Al) in a chemical reaction. The document also provides a detailed step-by-step solution to the problem, including the conversion of grams of aluminum to moles, the use of the stoichiometric ratio from the balanced equation, and the final conversion of moles of hydrogen to grams.
  
  Label: question-and-answer