Westonci.ca is your trusted source for finding answers to a wide range of questions, backed by a knowledgeable community. Get detailed answers to your questions from a community of experts dedicated to providing accurate information. Our platform provides a seamless experience for finding reliable answers from a network of experienced professionals.
Sagot :
Certainly! Let's balance the chemical equation step by step:
The unbalanced chemical equation is:
[tex]\[ H_2 + O_2 \rightarrow H_2O \][/tex]
### Step 1: Count the number of atoms for each element on both sides.
- Reactants:
- Hydrogen ([tex]\(H\)[/tex]): 2 atoms (from [tex]\(H_2\)[/tex])
- Oxygen ([tex]\(O\)[/tex]): 2 atoms (from [tex]\(O_2\)[/tex])
- Products:
- Hydrogen ([tex]\(H\)[/tex]): 2 atoms (from [tex]\(H_2O\)[/tex])
- Oxygen ([tex]\(O\)[/tex]): 1 atom (from [tex]\(H_2O\)[/tex])
### Step 2: Balance the hydrogen atoms.
To balance the hydrogen atoms, we need to have the same number of hydrogen atoms on both sides. Currently, we have 2 hydrogen atoms in the reactants and 2 hydrogen atoms in the products. Thus, the hydrogen atoms are already balanced.
### Step 3: Balance the oxygen atoms.
To balance the oxygen atoms, we need to have the same number of oxygen atoms on both sides. Currently, we have 2 oxygen atoms in the reactants and 1 oxygen atom in the products.
Since there's only one [tex]\(O\)[/tex] in [tex]\(H_2O\)[/tex], we can try placing a coefficient of 2 in front of [tex]\(H_2O\)[/tex]:
[tex]\[ H_2 + O_2 \rightarrow 2 H_2O \][/tex]
### Step 4: Recount the number of atoms after adjusting coefficients.
- Reactants:
- Hydrogen ([tex]\(H\)[/tex]): 2 atoms (from [tex]\(H_2\)[/tex])
- Oxygen ([tex]\(O\)[/tex]): 2 atoms (from [tex]\(O_2\)[/tex])
- Products:
- Hydrogen ([tex]\(H\)[/tex]): 4 atoms (from 2 [tex]\(H_2O\)[/tex])
- Oxygen ([tex]\(O\)[/tex]): 2 atoms (from 2 [tex]\(H_2O\)[/tex])
### Step 5: Balance the hydrogen atoms again.
We now see that we have 4 hydrogen atoms on the product side but only 2 hydrogen atoms on the reactant side. To balance the hydrogen atoms, we need to place a coefficient of 2 in front of [tex]\(H_2\)[/tex]:
[tex]\[ 2 H_2 + O_2 \rightarrow 2 H_2O \][/tex]
### Step 6: Final check.
- Reactants:
- Hydrogen ([tex]\(H\)[/tex]): 4 atoms (from 2 [tex]\(H_2\)[/tex])
- Oxygen ([tex]\(O\)[/tex]): 2 atoms (from [tex]\(O_2\)[/tex])
- Products:
- Hydrogen ([tex]\(H\)[/tex]): 4 atoms (from 2 [tex]\(H_2O\)[/tex])
- Oxygen ([tex]\(O\)[/tex]): 2 atoms (from 2 [tex]\(H_2O\)[/tex])
Now the equation is balanced on both sides, with 4 hydrogen atoms and 2 oxygen atoms.
Therefore, the coefficients required to balance the equation are:
- [tex]\(2\)[/tex] in front of [tex]\(H_2\)[/tex]
- [tex]\(2\)[/tex] in front of [tex]\(H_2O\)[/tex]
So, the balanced chemical equation is:
[tex]\[ 2 H_2 + O_2 \rightarrow 2 H_2O \][/tex]
Hence, the coefficients to be placed in front of [tex]\(H_2\)[/tex] and [tex]\(H_2O\)[/tex] are both:
[tex]\[ \boxed{2} \][/tex]
The unbalanced chemical equation is:
[tex]\[ H_2 + O_2 \rightarrow H_2O \][/tex]
### Step 1: Count the number of atoms for each element on both sides.
- Reactants:
- Hydrogen ([tex]\(H\)[/tex]): 2 atoms (from [tex]\(H_2\)[/tex])
- Oxygen ([tex]\(O\)[/tex]): 2 atoms (from [tex]\(O_2\)[/tex])
- Products:
- Hydrogen ([tex]\(H\)[/tex]): 2 atoms (from [tex]\(H_2O\)[/tex])
- Oxygen ([tex]\(O\)[/tex]): 1 atom (from [tex]\(H_2O\)[/tex])
### Step 2: Balance the hydrogen atoms.
To balance the hydrogen atoms, we need to have the same number of hydrogen atoms on both sides. Currently, we have 2 hydrogen atoms in the reactants and 2 hydrogen atoms in the products. Thus, the hydrogen atoms are already balanced.
### Step 3: Balance the oxygen atoms.
To balance the oxygen atoms, we need to have the same number of oxygen atoms on both sides. Currently, we have 2 oxygen atoms in the reactants and 1 oxygen atom in the products.
Since there's only one [tex]\(O\)[/tex] in [tex]\(H_2O\)[/tex], we can try placing a coefficient of 2 in front of [tex]\(H_2O\)[/tex]:
[tex]\[ H_2 + O_2 \rightarrow 2 H_2O \][/tex]
### Step 4: Recount the number of atoms after adjusting coefficients.
- Reactants:
- Hydrogen ([tex]\(H\)[/tex]): 2 atoms (from [tex]\(H_2\)[/tex])
- Oxygen ([tex]\(O\)[/tex]): 2 atoms (from [tex]\(O_2\)[/tex])
- Products:
- Hydrogen ([tex]\(H\)[/tex]): 4 atoms (from 2 [tex]\(H_2O\)[/tex])
- Oxygen ([tex]\(O\)[/tex]): 2 atoms (from 2 [tex]\(H_2O\)[/tex])
### Step 5: Balance the hydrogen atoms again.
We now see that we have 4 hydrogen atoms on the product side but only 2 hydrogen atoms on the reactant side. To balance the hydrogen atoms, we need to place a coefficient of 2 in front of [tex]\(H_2\)[/tex]:
[tex]\[ 2 H_2 + O_2 \rightarrow 2 H_2O \][/tex]
### Step 6: Final check.
- Reactants:
- Hydrogen ([tex]\(H\)[/tex]): 4 atoms (from 2 [tex]\(H_2\)[/tex])
- Oxygen ([tex]\(O\)[/tex]): 2 atoms (from [tex]\(O_2\)[/tex])
- Products:
- Hydrogen ([tex]\(H\)[/tex]): 4 atoms (from 2 [tex]\(H_2O\)[/tex])
- Oxygen ([tex]\(O\)[/tex]): 2 atoms (from 2 [tex]\(H_2O\)[/tex])
Now the equation is balanced on both sides, with 4 hydrogen atoms and 2 oxygen atoms.
Therefore, the coefficients required to balance the equation are:
- [tex]\(2\)[/tex] in front of [tex]\(H_2\)[/tex]
- [tex]\(2\)[/tex] in front of [tex]\(H_2O\)[/tex]
So, the balanced chemical equation is:
[tex]\[ 2 H_2 + O_2 \rightarrow 2 H_2O \][/tex]
Hence, the coefficients to be placed in front of [tex]\(H_2\)[/tex] and [tex]\(H_2O\)[/tex] are both:
[tex]\[ \boxed{2} \][/tex]
We hope our answers were helpful. Return anytime for more information and answers to any other questions you may have. Thanks for using our service. We're always here to provide accurate and up-to-date answers to all your queries. Westonci.ca is your go-to source for reliable answers. Return soon for more expert insights.
