Question

what you may notice in all of these reactions is that the relative number of molecules or moles stays the same. there will always be twice as many h₂ molecules as o₂ molecules in the balanced equation. there will always be the same number of h₂ molecules as h₂o molecules. this is because stoichiometric coefficients represent the relative number of molecules that participate in a reaction. based on the ratio of the balanced chemical reaction, insert a number in the blanks below. 150000 molecules o₂ + h₂ → h₂o mol o₂ + 6 h₂ → h₂o

Explanation:

Step1: Determine the stoichiometric ratio

The balanced chemical equation for the reaction between \(H_2\) and \(O_2\) to form \(H_2O\) is \(2H_2+O_2 = 2H_2O\). The ratio of \(H_2\) to \(O_2\) is \(2:1\), and the ratio of \(H_2\) to \(H_2O\) is \(1:1\).

Step2: Calculate the number of \(H_2\) molecules

Given \(150000\) \(O_2\) molecules. Since the ratio of \(H_2\) to \(O_2\) is \(2:1\), the number of \(H_2\) molecules is \(2\times150000 = 300000\).

Step3: Calculate the number of \(H_2O\) molecules

Since the ratio of \(H_2\) to \(H_2O\) is \(1:1\), the number of \(H_2O\) molecules is equal to the number of \(H_2\) molecules, which is \(300000\).

Step4: Calculate the number of \(O_2\) moles

Given \(6\) \(H_2\) moles. Since the ratio of \(H_2\) to \(O_2\) is \(2:1\), the number of \(O_2\) moles is \(\frac{6}{2}=3\).

Step5: Calculate the number of \(H_2O\) moles

Since the ratio of \(H_2\) to \(H_2O\) is \(1:1\), the number of \(H_2O\) moles is equal to the number of \(H_2\) moles, which is \(6\).

Answer:

For the first reaction: \(300000\) \(H_2\) molecules and \(300000\) \(H_2O\) molecules.
For the second reaction: \(3\) \(O_2\) moles and \(6\) \(H_2O\) moles.