For each of the following unbalanced equations, indicate how many moles of the first product are produced if 0.625 mol of the second product forms. State clearly the mole ratio used for each conversion.

Question

For each of the following unbalanced equations, indicate how many moles of the first product are produced if 0.625 mol of the second product forms. State clearly the mole ratio used for each conversion.

CH3CH2OH(l) + O2 --> CH3CHO(aq) + CH3CHO(aq) + H2O(l)

Answer 1

The equation and products along with the instructions are confusing. Does the "second product" refer to the second CH3CHO or to H2O. And since the equation is not balanced, is to be balanced before answering the question?

Answer 2

To determine how many moles of the first product are produced if 0.625 mol of the second product forms, we need to balance the equation first. The given equation is:

CH3CH2OH(l) + O2(g) -> CH3CHO(aq) + CH3CHO(aq) + H2O(l)

The mole ratio in the balanced equation will allow us to determine the moles of one substance relative to another. In this case, we want to find the amount of the first product in relation to the second product.

Let's balance the equation:

CH3CH2OH(l) + O2(g) -> 2CH3CHO(aq) + H2O(l)

Now that the equation is balanced, we can determine the mole ratio:

For every 2 moles of CH3CHO(aq) formed, 1 mole of CH3CH2OH(l) reacts.

This means:

1 mole CH3CH2OH(l) -> 2 moles CH3CHO(aq)

Now, since we know 0.625 mol of the second product (CH3CHO(aq)) forms, we can calculate the number of moles of the first product (CH3CH2OH(l)) produced.

Using the mole ratio, we have:

0.625 mol CH3CHO(aq) x (1 mole CH3CH2OH(l) / 2 moles CH3CHO(aq)) = 0.3125 mol CH3CH2OH(l)

Therefore, if 0.625 mol of the second product (CH3CHO(aq)) forms, 0.3125 mol of the first product (CH3CH2OH(l)) is produced.

Answer 3

To determine how many moles of the first product, CH3CHO(aq), are produced when 0.625 mol of the second product, H2O(l), forms, we need to balance the equation first.

The given unbalanced equation is:
CH3CH2OH(l) + O2 --> CH3CHO(aq) + CH3CHO(aq) + H2O(l)

To balance this equation, we need to ensure that there are equal numbers of atoms on both sides. Here's the balanced equation:
2 CH3CH2OH(l) + 6 O2 --> 2 CH3CHO(aq) + 2 CO2(g) + 6 H2O(l)

Now, let's determine the mole ratio between the first and second product. From the balanced equation, we can see that for every 2 moles of CH3CHO(aq) produced, 6 moles of H2O(l) are formed. Therefore, the mole ratio is:

1 mol of CH3CHO(aq) : 3 mol of H2O(l)

Since we have 0.625 mol of H2O(l), we can use this mole ratio to find the number of moles of CH3CHO(aq) produced. Let's calculate it:

0.625 mol of H2O(l) * (1 mol of CH3CHO(aq) / 3 mol of H2O(l)) = 0.208 mol of CH3CHO(aq)

Therefore, if 0.625 mol of H2O(l) forms, 0.208 mol of CH3CHO(aq) will be produced.

For each of the following unbalanced equations, indicate how many moles of the first product are produced if 0.625 mol of the second product forms. State clearly the mole ratio used for each conversion.

The equation and products along with the instructions are confusing. Does the "second product" refer to the second CH3CHO or to H2O. And since the equation is not balanced, is to be balanced before answering the question?

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To determine how many moles of the first product are produced if 0.625 mol of the second product forms, we need to balance the equation first. The given equation is:

To determine how many moles of the first product, CH3CHO(aq), are produced when 0.625 mol of the second product, H2O(l), forms, we need to balance the equation first.