E = mc²
where E = energy produced
m = mass of the nucleus
C = speed of light
m = 9.106 x 10⁻³ x 1.67 x 10⁻²⁷ kg
C = 3 x 10⁸ m/s, thus C² = 9 x 10¹⁶
E = 1.37 x 10⁻¹² J
The chemical equation can be expressed as:
2H2 + O2 = 2H2O
Given the amounts of the reactants, we need to identify the limiting reactant before calculating the amount of product generated.
4.0 g H2 ( 1 mol / 2.02 g ) = 1.98 mol H2
5.0 g O2 ( 1 mol / 32 g ) = 0.1563 mol O2
The limiting reactant is O2, as it will be fully consumed in the reaction.
0.1563 mol O2 ( 2 mol H2O / 1 mol O2 ) ( 18.02 g / mol ) = 5.6 g H2O will be produced
I hope you can decipher it and that it's also accurate. Wishing you all the best.
What precisely is being followed here?
