How many grams of oxygen and hydrogen is in water?

Hydrogen’s \% is therefore 2g/18g x 100 =11.1\%; oxygen’s is 16g/18g x 100 = 89.9\%; now, out of 100g of water, that makes 89.9g of oxygen and 11.1 g of hydrogen. Pradeep K.

How many grams of hydrogen are in 1g of water?

hydrogen is 2/18ths of the atomic mass of H2O. 2/18th of 36 is 4, so the answer is 4 grams.

How many grams of hydrogen and oxygen will need in 100 grams of water?

As the molar mass of hydrogen is 2, it requires 200/18 = 100/9 g of hydrogen. It requires 100/9 g of hydrogen gas and 800/9 g of oxygen gas to make 100 g of water.

Is 75 gram of water is decomposed how many grams of oxygen and hydrogen are obtained?

If we decompose 100 grams of pure water by passing electricity through it then 11 grams of hydrogen and 89 grams of oxygen obtained. This experiment shows that water always consists of the same two elements hydrogen and oxygen combine together in the same constant proportion of 11: 89 or 1:8 by mass.

How do you calculate hydrogen in grams of water?

To find the mass percent of hydrogen in water, take the molar mass of hydrogen in the water molecule, divide by the total molar mass of water, and multiply by 100. Dividing 2.016 by 18.016 gives you 0.1119. Multiply 0.1119 by 100 to get the answer: 11.19 percent.

How many grams are in oxygen?

For those elements that do not occur as single atoms – that is, the diatomic gases, sulfur, and phosphorus – it is important to be certain that you specify what you are talking about. One mole of atoms of oxygen has a mass of 16 g, as 16 is the atomic weight of oxygen, and contains 6.02 X 1023 atoms of oxygen.

How many grams of oxygen are there in water?

1. There are 16 grams of oxygen in 18 grams of water. We can see from the formula for water, H2O, there are twice as many hydrogen atoms (each of atomic mass 1) as oxygen atoms (each of atomic mass 16).

When 18 grams of water decomposes the products are?

​As 18 g of water is decomposed. 1 mole of water or 18 g of water produces 0.5 mole of Oxygen gas. 0.5 mole of Oxygen gas is equivalent to 16 g of Oxygen gas. 18 g of water decomposed to produce 16 g of Oxygen gas.

What mass of water can be produced from 10 grams of hydrogen?

Since oxygen is in excess, it implies that hydrogen is the limiting reagent and will decide how much product is formed, according to the mole ratio of the balanced equation. nH2=mMr=10.10g2g/mol=5.05mol .

How do you find the percentage of hydrogen and oxygen in water?

For example, to find the ratio of mass of hydrogen to oxygen in water, divide the total molar mass of hydrogen, 2.016, by the molar mass of oxygen, 16.00 and get 0.126. To find the ratio of oxygen to hydrogen, divide 16.00 by 2.016 and get 7.937. This means in water, oxygen outweighs hydrogen by almost 8 to 1.

How many molecules of water are in 9 grams of water?

Water has 18 grams per mole so 9 grams is 0.5 moles of water. There are 6.022* 10^23 molecules in a mole. Each water molecule contains *one* oxygen and *two* hydrogens. SO! We have in 9 grams of water.

What is the molecular weight of H2O in grams?

Going by the common average atomic weights on the periodic table (average isotope distribution), oxygen has an atomic weight of 15.999 and hydrogen rings in at 1.008. So water has a molecular weight of 18.15, and going to the same third decimal place you will create 18.016 grams of H2O from 16.0 grams of oxygen and 4.0 grams of hydrogen.

How do you calculate the percentage of hydrogen and oxygen in water?

You need to determine the percent by mass of both hydrogen and oxygen in water. Since the formula for water is H2O, take the masses off of the periodic table: 2x1g for hydrogen (because there are 2 H in the formula); 1x 16g for oxygen (because there is 1 O in the formula), added together for a total of 18g.

What happens when 8g of H2 reacts with 64g of oxygen?

1 g H2 reacts with= 8 g Oxygen. So 64 g of oxygen reacts with= 8 g H2. So (64+8)=72 g of water will be formed. Now (70–64)= 6 g of oxygen will remain unreacted. So finally to say when 8 g of H2 reacts with oxygen, 8 times that of hydrogen, ie 64 g will react and the remaining 6 g will remain unreacted.