Respuesta :
Answer : The rate of consumption of oxygen = 0.245 mol/s
Solution : Given,
Rate at which Hydrogen burns = 0.49 mol/s
The Reaction is,
[tex]2H_{2}(g)+O_{2}(g)\rightarrow 2H_{2}O(l)[/tex]
In this reaction, 2 moles of hydrogen react with the 1 mole of oxygen.
The rate at which oxygen burns is equal to the half of rate at which hydrogen burns.
Rate at which Oxygen burns = [tex]\frac{1}{2}[/tex] × 0.49 mol/s
= 0.245 mol/s
The study of chemicals and bonds s called chemistry. There are different types of chemical reactions and these are combination reaction, decomposition reaction and etc.
The correct answer is The rate of consumption of oxygen = 0.245 mol/s
What is a combination reaction?
When one or more elements of reactant join together to form a single compound is called a combination reaction.
Rate at which Hydrogen burns = 0.49 mol/s
The Reaction is,
- [tex]2h_2(g)+o_2(g)---->2h_2o(g).[/tex]
In this reaction, 2 moles of hydrogen react with 1 mole of oxygen.
The rate at which oxygen burns is equal to half of the rate at which hydrogen burns.
The ratee at which Oxygen burns = 1/2 × 0.49 mol/s
= 0.245 mol/s
Hence, the correct answer is 0.245mol/s.
For more information about the reaction, refer to the link:-
https://brainly.in/question/9531558
