Ok we trying this again. so just in case if the picture isnt showing, here are the questions: 1. Given the unbalanced equation:
C12H22O11 = C + H2O
If you produced 34.55 moles of C, how many moles of water were produced as well?

2. Given the unbalanced equation:
Cr + H2SO4 = CrSO4 + H2
If you want to make 14.81 moles of CrSO4, how many moles of Cr do you need?

1. 31.68 moles of water, H₂O

2. 14.81 moles of Cr

Explanation:

1. Determination of the number of mole of water, H₂O.

The balanced equation for the reaction is given below:

C₁₂H₂₂O₁₁ —> 12C + 11H₂O

From the balanced equation above,

1 mole of C₁₂H₂₂O₁₁ produced 12 moles of C and 11 moles of H₂O.

Next, we shall determine the number of mole C₁₂H₂₂O₁₁ needed to produce 34.55 moles of C. This can be obtained as follow:

From the balanced equation above,

1 mole of C₁₂H₂₂O₁₁ produced 12 moles of C.

Therefore, Xmol of C₁₂H₂₂O₁₁ will produce 34.55 moles of C i.e

Xmol of C₁₂H₂₂O₁₁ = 34.55 / 12

Xmol of C₁₂H₂₂O₁₁ = 2.88 moles

Thus, 2.88 moles of C₁₂H₂₂O₁₁ is needed.

Finally, we shall determine the number of mole of water, H₂O produced from the reaction. This can be obtained as follow:

From the balanced equation above,

1 mole of C₁₂H₂₂O₁₁ produced 11 moles of H₂O.

Therefore, 2.88 moles of C₁₂H₂₂O₁₁ will produce = 2.88 × 11 = 31.68 moles of H₂O.

Thus, 31.68 moles of water, H₂O were obtained from the reaction.

2. Determination of the number of mole of Cr needed.

The balanced equation for the reaction is given below:

Cr + H₂SO₄ —> CrSO₄ + H₂

From the balanced equation above,

1 mole of Cr reacted to produce 1 mole of CrSO₄.

Finally, we shall determine the number of mole of Cr needed to produce 14.81 moles of CrSO₄. This can be obtained as follow:

From the balanced equation above,

1 mole of Cr reacted to produce 1 mole of CrSO₄.

Therefore, 14.81 moles of Cr will also react to produce 14.81 moles of CrSO₄.

Thus, 14.81 moles of Cr is needed for the reaction.

is there any options? maybe im just not seeing them but i need the options to

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