Using the following equation 2c2h6 +7o2 --> 4co2 +6h2o if 9.5g c2h6 react with 130g of o2, how many grams of water will be produced? question options: 32 41 9 17

Answer : The mass of produced will be, 17 grams.

Explanation : Given,

Mass of = 9.5 g

Mass of = 130 g

Molar mass of = 30 g/mole

Molar mass of = 32 g/mole

Molar mass of = 18 g/mole

First we have to calculate the moles of and .

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

From the balanced reaction we conclude that

As, 2 moles of react with 7 mole of

So, 0.317 moles of react with moles of

From this we conclude that, is an excess reagent because the given moles are greater than the required moles and is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of .

As, 2 moles of react to give 6 moles of

So, 0.317 moles of react to give moles of

Now we have to calculate the mass of .

Therefore, the mass of produced will be, 17 grams.

"hydrogen bonding is the attraction of h atoms in the water molecule (slight + charge) to o atoms in a neighboring water molecule (slight - charge); it is a weak interatomic force. but it is still strong enough to the water molecules "stick" together."

answer: they produce more slow than unicellular organisms.