Asked by THING1
Refer to the scenario and balanced equation.
2H2 + O2 → 2H2O
At the beginning of the reaction, it is measured that there are 15.0 g of hydrogen (H2) and 97.0 g of oxygen (O2).
What is the theoretical yield for the water that will be produced in the reaction? (M H2O = 18.0 g/mol; M CH4 = 16.0 g/mol)
5.38 x 100 g H2O
1.34 x 102 g H2O
1.08 x 102 g H2O
2.73 x 101 g H2O
2H2 + O2 → 2H2O
At the beginning of the reaction, it is measured that there are 15.0 g of hydrogen (H2) and 97.0 g of oxygen (O2).
What is the theoretical yield for the water that will be produced in the reaction? (M H2O = 18.0 g/mol; M CH4 = 16.0 g/mol)
5.38 x 100 g H2O
1.34 x 102 g H2O
1.08 x 102 g H2O
2.73 x 101 g H2O
Answers
Answered by
THING1
PLEASE IM DESPERATE!!!!!
Answered by
timmy tenders
Hydrogen and oxygen can react to form water. This reaction produces a lot of heat energy. 2H2 + O2 → 2H2O While this reaction is thermodynamically feasible (i.e. water has a much lower free energy than the hydrogen/oxygen mixture), there is a large kinetic (activation energy) barrier to the reaction happening.
is what i found to maybe help u its not the answer but itll help
is what i found to maybe help u its not the answer but itll help
Answered by
timmy tenders
n also im in 7th
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