What mass of water can be made if 6.00 grams of hydrogen reacts with 40.00 grams of oxygen?

Answer 1

46 grams of water.

number of mols (n) = mass/molecular weight

for: 2H2 + O2 -> 2H2O

n(H2) = 6 grams/ (2 grams/mol)

= 3 mol

n(O2) = 40 grams/(16 grams/mol)

= 2.5mol

So you can make a maximum of 2.5mol of water.

2.5 mol * 18 g/mol = 46 grams water.

Answer 2

The answer would be 4.8 because during any chemical reaction, the mass of the product is always equal to the mass of the reactants. Therefore, since hydrogen is the product, the answer will be 4.8 grams.

Answer 3

The formula of water is H2O, showing that two atoms of hydrogen are required for each atom of oxygen in water. The gram Atomic Mass for hydrogen is 1.008, and the gram atomic mass for oxygen is 15.9994. Therefore 4.00 grams of hydrogen constitutes 4.00/1.008 or 3.97 gram atomic masses of hydrogen, while 4.00 grams of oxygen constitutes only 4.00/15.9994 or 0.250 gram atomic masses of oxygen. Oxygen is therefore the limiting element in this reaction, and only 0.500 gram atomic masses of hydrogen can be reacted with the available amount of oxygen. The grams of water formed will be [4.00 + (0.500)(1.008)] or a total of 4.50 grams of water, to the justified number of significant digits.

Answer 4

Balanced equation: 2H2(g) + O2(g) ---> 2H2O(g)

moles of H2 added = 4 g x 1 mol/2 g = 2 moles H2

moles O2 added = 32 g x 1 mol/32 g = 1 mole O2

Since the H2 and O2 are present in a 2:1 mole ratio, this is the same as in the balanced equation.

Thus, as can also been seen in the balanced equation, 2 moles of H2O will be produced.

Mass of H2O produced = 2 moles H2O x 18 g/mole = 36 grams <--- answer

NOTE: This can also be seen by the fact that 4 g H2 + 32 g O2 = 36 g total mass of product. This is an example of the Law of Conservation of Matter.

Answer 5

43.2 grams of water

Answer 6

43.2 grams of water

Answer 7

5,7 g oxygen reacted.

Answer 8

\

Answer 9

7.2