Calculate the energy required to ionize a ground state hydrogen atom. report your answer in kilojoules. socratic. org

           ΔE  =  2.18 × 10⁻²¹ kJ

Using Bohr Energy Equation,

                                    ΔE  =  - R (1/nₐ² - 1/nₓ²)

Where;

           R  =  Rydberg's constant  =  2.18 × 10⁻¹⁸ J

           nₐ  =  Infinity  =  ∞   (electron removed from H atom)

           nₓ  =  1   (Ground state of H atom)

Putting Values in equation 1,

                                    ΔE  =  - 2.18 × 10⁻¹⁸ J × ( 1/∞² - 1/1²)

                                    ΔE  =  - 2.18 × 10⁻¹⁸ J × ( 0 - 1)

                                    ΔE  =  - 2.18 × 10⁻¹⁸ J × (-1)

                                    ΔE  =  2.18 × 10⁻¹⁸ J

                                    ΔE  = 2.18 × 10⁻²¹ kJ

fe 55.85 g/mol and h2o 18.02 g/mol.

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.