Question

in the final chemical equation, nacl and o2 are the products that are formed through the reaction between na2o and cl2. before you can add these intermediate chemical equations, you need to alter them by multiplying the first equation by 2. multiplying the second equation by (1/4). multiplying the first equation by (1/2). multiplying the second equation by 2.

Explanation:

Step1: Analyze chemical - equation combination

To combine intermediate chemical equations to get a final equation with products NaCl and O₂ from Na₂O and Cl₂, we need to balance the atoms on both sides of the combined equation. Usually, we multiply the equations to make the number of certain atoms match.
Let's assume the two intermediate equations are:
Equation 1: \(aNa_2O + bCl_2
ightarrow cNaCl + dO_2\)
Equation 2: \(eNa_2O + fCl_2
ightarrow gNaCl + hO_2\)
We know that in the final equation, we want to balance the sodium (Na), chlorine (Cl) and oxygen (O) atoms.
The reaction of \(Na_2O\) and \(Cl_2\) to form \(NaCl\) and \(O_2\) has the general un - balanced form \(Na_2O+Cl_2
ightarrow NaCl + O_2\). Balancing this equation gives \(2Na_2O + 4Cl_2=4NaCl+O_2\).
If we have two intermediate equations, we need to adjust them so that when added, the atoms are balanced.
If we assume one of the intermediate equations has a coefficient mismatch for a particular atom, we multiply the equations to correct it.
Let's assume the first intermediate equation has a lower number of sodium or chlorine atoms compared to the final - balanced equation requirements. Multiplying the first equation by 2 can help in balancing the atoms when the two intermediate equations are added.

Step2: Evaluate options

• Multiplying the first equation by 2 can help in balancing the number of sodium and chlorine atoms in the combined equations to get the final balanced equation for the reaction of \(Na_2O\) and \(Cl_2\) to form \(NaCl\) and \(O_2\).
• Multiplying the second equation by \(\frac{1}{4}\) or \(\frac{1}{2}\) will not help in getting integer - valued coefficients for the final balanced equation. Multiplying the second equation by 2 may not be the correct step as the key step is often to adjust the first equation to match the stoichiometry of the final reaction.

Answer:

multiplying the first equation by 2.