How many moles of carbon tetrahydride are needed to produce 3.59 moles of water
To determine the number of moles of carbon tetrahydride (CH4) needed to produce a certain number of moles of water (H2O), we need to refer to the balanced chemical equation representing the reaction between carbon tetrahydride and water.
Since we don't have the balanced equation provided, let's consider the balanced equation for the combustion of methane (CH4):
CH4 + 2O2 -> CO2 + 2H2O
From this equation, we can see that for every 1 mole of methane (CH4), we get 2 moles of water (H2O). This means that the molar ratio between CH4 and H2O is 1:2.
Now, if we have 3.59 moles of water (H2O), we can determine the number of moles of carbon tetrahydride (CH4) needed using the molar ratio mentioned above.
By multiplying the number of moles of water (3.59 moles) by the molar ratio (1 mole CH4 / 2 moles H2O), we can find the number of moles of carbon tetrahydride needed.
3.59 moles H2O * (1 mole CH4 / 2 moles H2O) = 1.795 moles CH4
So, 1.795 moles of carbon tetrahydride are needed to produce 3.59 moles of water.