A) balanced chemical equation for the formation of liquid water from gaseous hydrogen and gaseous oxygen?
B) balanced equations of the formation of liquid water from gaseous hydrogen and gaseous oxygen?
C) balanced equation for the combustion of metal to form 1 mole of magnesium?
Can some one help balance these ?????
B) balanced equations of the formation of liquid water from gaseous hydrogen and gaseous oxygen?
C) balanced equation for the combustion of metal to form 1 mole of magnesium?
Can some one help balance these ?????
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The formula for water is H2O.
Hydrogen (H2) and oxygen (O2) are among the diatomic elements (HNOF BrICl, enough brickle)
So A and B are 2H2(g) + O2(g) ---> 2H2O(l)
g = gas, l = liquid
I don't think C is possible. One mole of metal magnesium can combust, but it is a reactant, not a product. It will form a mole of magnesium oxide.
Mg + ½O2 ---> MgO
It is not uncommon, particularly in thermodynamic calculations, for oxygen to have a fractional coefficient. That way the equation can be written for one mole of fuel.
Hydrogen (H2) and oxygen (O2) are among the diatomic elements (HNOF BrICl, enough brickle)
So A and B are 2H2(g) + O2(g) ---> 2H2O(l)
g = gas, l = liquid
I don't think C is possible. One mole of metal magnesium can combust, but it is a reactant, not a product. It will form a mole of magnesium oxide.
Mg + ½O2 ---> MgO
It is not uncommon, particularly in thermodynamic calculations, for oxygen to have a fractional coefficient. That way the equation can be written for one mole of fuel.
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A) 2H2(g) + O2(g) >>>>>>>>>>>>>> 2H2O(l)
B) 2H2(g) + O2(g) >>>>>>>>>>>>>> 2H2O(l)
C) doesn't make any sense
B) 2H2(g) + O2(g) >>>>>>>>>>>>>> 2H2O(l)
C) doesn't make any sense