The balanced chemical equation for the reaction between oxygen and hydrogen is
2H2 + 02 -> 2H2O
Thus 2.2 moles of oxygen reacts with 4.4 moles of hydrogen to form 4.4 moles of steam (water in gaseous state).
The mass of H2O obtained is thus 4.4 x 18.0 = 79.2g.
The reaction is 2H2 + O2-> 2H2O So, both the molar and volume ratios would be 2 moles(liters) of hydrogen to every mole(liter) of oxygen. By weight, the ratio would be about 8 grams of oxygen to every gram of hydrogen
340 grams
lets see. H20 you have 2.016 grams of hydrogen here to 16.0 grams oxygen 2.016/16.0 X 100 = 12.6% hydrogen by mass H2O2 you have the same 2.016 grams hydrogen here, but you have 32.0 grams oxygen in this molecule 2.016/32.0 X 100 = 6.3% so H2O has the higher percent by mass of hydrogen
5.36 g
Answer: 16 g of oxygen and 2 g of hydrogen.
25
Also 10 grams.
Also 10 grams.
The percentage of oxygen is 54,84 %.
The reaction is 2H2 + O2-> 2H2O So, both the molar and volume ratios would be 2 moles(liters) of hydrogen to every mole(liter) of oxygen. By weight, the ratio would be about 8 grams of oxygen to every gram of hydrogen
In chemistry, the outcome of a reaction must have the same mass as the initial state. This means that if you have 32g of oxygen and 4g of hydrogen, you just have to add the numbers to discover the original mass (in this case, 36g).
It is not measured in grams but PPM because it is a gas.
what is the mass in grams of oxygen, is needed to complete combustion of 6 L of methane?
340 grams
lets see. H20 you have 2.016 grams of hydrogen here to 16.0 grams oxygen 2.016/16.0 X 100 = 12.6% hydrogen by mass H2O2 you have the same 2.016 grams hydrogen here, but you have 32.0 grams oxygen in this molecule 2.016/32.0 X 100 = 6.3% so H2O has the higher percent by mass of hydrogen
43.2 grams of water
5.36 g