H2+1/2O2=H2O(1)+285.8kj
this exothermic or endothermic why because and with formula
You need to learn how to write a question. The equation is exothermic because it is giving off 285.8 kJ of heat.
If the energy number is on the product side of the equation, it is exothermic as the one you've posted. If the energy number is on the reactant side of the equation, it is endothermic. => H₂O(l) + 44Kj => H₂O(g)
H2(g)+1/2O(g)~H2O(1)+285.8kj
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The chemical equation you provided represents the reaction of hydrogen gas (H2) combining with half the amount of oxygen gas (O2) to form water (H2O) with the release of 285.8 kilojoules (kJ) of energy.
To understand how to get the answer, let's break down the given equation step by step:
1. H2 represents two moles of hydrogen gas, and 1/2O2 represents 0.5 moles of oxygen gas. In a balanced chemical equation, the coefficients represent the number of moles of each reactant and product.
2. By combining two moles of hydrogen gas with 0.5 moles of oxygen gas, the reaction forms one mole of water (H2O).
3. The equation also states that this reaction releases 285.8 kJ of energy. The energy is given as a product, indicating that it is being released during the reaction.
To calculate the energy released during the reaction, you need to know the enthalpy change (ΔH) associated with the formation of one mole of water. In this case, the ΔH is -285.8 kJ. The negative sign indicates that the reaction is exothermic (releasing energy).
Therefore, when one mole of water is formed, it releases 285.8 kJ of energy. If you have a different quantity of water being formed, you can use stoichiometry to determine the energy released. Just multiply the amount of water in moles by the given energy value per mole (-285.8 kJ) to find the corresponding energy.
Keep in mind that this explanation assumes all reactants and products are in their standard states and that the reaction occurs at constant pressure. Additional factors, such as temperature and pressure, can affect the actual energy release in a reaction.