The reaction cao(s)+ h2o(> ca(oh)2 delta h= -65.2 kj

how much energy will be released if 500.0g of cao is reacted

There is 582 kJ of energy released. Δ H rxn  for 500g=  −  582 kJ  ( negative because the energy is released).

Explanation:

Step 1: The balanced equation

CaO(s)+ H2O(l) → ca(OH)2     ΔH= -65.2 kJ

In this situation, 1 mole of CaO consumed, needs 1 mole of H2O to produce 1 mole of Ca(OH)2

The enthalpy change of this reaction is  Δ H rxn =  −  65.2 kJ

This means the reaction gives off  65.2 kJ  of heat when 1 mole of CaO and 1 mole of H2O react.

Step 2: Calculate number of moles in 500 g of CaO

Number of moles = mass of CaO / Molar mass of CaO

Number of moles = 500 grams / 56.077 g/mol = 8.92 moles

Step 3: Calculate energy released

Since there is released 65.2 kJ when 1 mole of CaO reacts; for 8.92 moles of CaO there will be released 8.92 * 65.2 kJ = 581.584 ≈ 582 kJ

.

There is given off 582 kJ of energy

Δ H rxn  for 500g=  −  582 kJ

it is to be noted that an alpha particle is an helium nucleus. so it contains 2 protons 2 neutrons and has a mass number of 4. when alpha decay particles are ejected from the nucleus it gets transformed into an atom which has atomic number less than 2 and a mass number less than 4.

an equation that could represent alpha decay is radium 226 decay of alpha particle forms radon 222.

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- lead + phosphoric acid = hydrogen + lead(ii) phosphate