Question

Hydrogen and oxygen react chemically to form water. How much water would form if \[4.8\] grams of hydrogen reacted with \[38.4\] grams of oxygen?

Answer 1

Hint: At the point when atomic hydrogen and oxygen are consolidated and permitted to react together, energy is delivered and the particles of hydrogen and oxygen can join to frame either water or hydrogen peroxide. These two cycles are represented by the two chemical equations. Scientists use redox half-reactions to portray thermodynamic cycles.

Complete step-by-step answer: First we would need to calculate the empirical formula (lowest mole ratio of atoms) this can be done by simply finding the ratio of moles given. We know that \[H\] and \[O\] react to create water (unknown formula), and we know that \[H\] has a \[ + 1\] charge while \[O\] has a \[ - 2\] charge. So if they were to create a neutral molecule it would need two \[H\] forever one \[O\].
So we have a ratio to work with, now we can convert grams to moles and we get grams of sample/molar mass of element (g/mole) = moles of element
\[\dfrac{{4.8gH}}{{1g/moleH}} = 4.8molesH\]
 (\[2H\] Are needed for proper ratio so, \[\dfrac{{4.8}}{2} = 2.4moleperH\])
\[\dfrac{{38.4gO}}{{16g/mole}} = 2.4molesofO\]
Now, the ratio of \[H\] to \[O\] is\[2 - 1\], just like the ratio. Now since the moles given are even in ratio, and we know the moles of one of the reactants we can calculate moles of product. Which will equal \[2.4moles{H_2}O\].

Note: Chemical reaction, a cycle where at least one substance, the reactants, are changed over to at least one unique substance, the products. Substances are either synthetic components or compounds. A chemical reaction adjusts the constituent molecules of the reactants to make various substances as products.