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1. Consider this reaction:

H₂(g) +   O₂ (g)     à      H₂O (g)                                       dHo = __________

1. Balance the equation and put the correct number of moles in theequation above. (1 point)

1. Classify the forward reaction as (1) Combustion, (2)Decomposition, (3) Single replacement, (4) Double replacement, (5)Neutralization, (6) Synthesis. Circle the correct answer. (1point)

1. In this reaction did Hydrogen get oxidized or reduced? Circlethe correct answer. (1 point)

1. Based on your answer above is Hydrogen an oxidizing or reducingreactant? Circle the correct answer. (1 point)

1. In this reaction did Oxygen get oxidized or reduced? Circle thecorrect answer. (1 point)

1. Based on the answer above, is Oxygen an oxidizing or reducingagent? Circle the correct (1 point)
   
2. Calculate the dHo of the Synthesis reaction using thevalues from the table in Appendix 2. Show your work.(2 points)

1. If 4 moles of H2 is used in a balanced equation for thesynthesis reaction, how many moles of water will be produced(without using the tables). Show your work. (1 point)

1. If 4 moles of H2 is used for the Synthesis reaction, calculatethe enthalpy of the reaction without using the tables. Show yourwork. (1 point)

1. If 4 moles of H₂O is required to be produced, howmany moles of H₂ and how many moles of O₂will be required (without using tables). Show your work. (1point).

1. If 1 mole of water is required to be produced, how many molesof H₂ and O₂ will be required (without usingtables)? Show your work. (1 point)

1. If 6 moles of water is decomposed, how many moles ofH₂ and O₂ will be formed? (1point)

1. If 6 moles of water is decomposed, calculate the enthalpy ofthe reaction without using the values from the table available inAppendix 2 of your textbook. (2 points)