Answered

Explore Westonci.ca, the top Q&A platform where your questions are answered by professionals and enthusiasts alike. Get accurate and detailed answers to your questions from a dedicated community of experts on our Q&A platform. Join our Q&A platform to connect with experts dedicated to providing accurate answers to your questions in various fields.

How many grams of water will be produced if you start with 4.0 grams of hydrogen and an excess of oxygen given the following balanced chemical equation?

2H2 + O2 → 2H2O

Group of answer choices

A. 32.0 grams

B. 36.0 grams

C. 54.0 grams

D. 18.0 grams

Sagot :

CrystalQueen

Answer:

B.) 36.0 grams

Explanation:

To find the mass of water, you need to (1) convert grams H₂ to moles (using the molar mass), then (2) convert moles H₂ to moles H₂O (using mole-to-mole ratio from reaction coefficients), and then (3) convert moles H₂O to grams (using the molar mass). It is important to arrange the conversions in a way that allows for the cancellation of units.

Molar Mass (H₂): 2(1.008 g/mol)

Molar Mass (H₂): 2.016 g/mol

Molar Mass (H₂O): 2(1.008 g/mol) + 15.998 g/mol

Molar Mass (H₂O): 18.014 g/mol

2 H₂ + O₂ -----> 2 H₂O
^                        ^

4.0 g H₂            1 mole             2 moles H₂O           18.014 g
---------------  x  ----------------  x  ------------------------  x  ---------------  = 36 g H₂O
                          2.016 g             2 moles H₂              1 mole

Thanks for stopping by. We are committed to providing the best answers for all your questions. See you again soon. We hope you found this helpful. Feel free to come back anytime for more accurate answers and updated information. Your questions are important to us at Westonci.ca. Visit again for expert answers and reliable information.