how many grams of H2O are needed to react completely with 3.5 moles of ethylene?

I THINK that the reaction is a 1 to 1 mole reaction , so you should need 3.5 moles of H2O.

3.5 moles of H2O*(18.00g/1 mole)= mass of H2O

***2-significant figures.

Like I said, I think 3.5 moles of H2O is needed.

To determine the number of grams of H2O needed to react completely with 3.5 moles of ethylene (C2H4), we need to use the balanced chemical equation for the reaction between ethylene and water.

The balanced equation for the reaction is:
C2H4 + H2O → C2H5OH

From the equation, we can see that 1 mole of ethylene (C2H4) reacts with 1 mole of water (H2O) to produce 1 mole of ethanol (C2H5OH).

First, we need to calculate the molar mass of H2O:
H2O = 2(1.008 g/mol) + 16.00 g/mol = 18.02 g/mol

Now, we can determine the number of grams of H2O needed using the following steps:
1. Calculate the number of moles of H2O needed:
3.5 moles of C2H4 × 1 mole of H2O/1 mole of C2H4 = 3.5 moles of H2O

2. Convert moles of H2O to grams:
3.5 moles of H2O × 18.02 g/mol = 63.07 grams of H2O

Therefore, 63.07 grams of H2O are needed to react completely with 3.5 moles of ethylene.