Oxygen difluoride is an unstable molecule that reacts readily with water. calculate the bond energy of the o–f bond using the standard enthalpy of reaction and the bond energy data provided. just enter a number (no units). of2(g) + h2o(g) \longrightarrow ⟶ o=o(g) + 2hf(g) \delta δ h° = –318 kj bond: o–h o=o h–f bond energy (kj/mol): 467 498 565

Someone offer some answers to this, i will give 98 coins and mark as brainliest! i will put the rest of the lab down in the comments,solutions pre-lab questions: in this lab, you will make fruit drinks with powdered drink mix. complete the pre-lab questions to get the values you need for your drink solutions. calculate the molar mass of powered fruit drink mix, made from sucrose (c12h22o11).using stoichiometry, determine the mass of powdered drink mix needed to make a 1.0 m solution of 100 ml. (hint: use molarity = to find the moles of drink mix, then convert moles to grams using a mole conversion.)what mass of powdered drink mix is needed to make a 0.5 m solution of 100 ml?

Place the elements below in order of decreasing ionization energy. aluminum(al) chlorine(cl) magnesium (mg) sulfur(s)

The table compares the number of electrons in two unknown neutral atoms. comparison of electrons atom number of electrons a 9 d 11 use this information to determine the number of valence electrons in the atoms. which of the following correctly compares the stability of tthe table compares the number of electrons in two unknown neutral atoms. comparison of electrons atom number of electrons a 9 d 11 use this information to determine the number of valence electrons in the atoms. which of the following correctly compares the stability of the two atoms? both are unreactive. both are highly reactive. a is unreactive and d is reactive. a is reactive and d is unreactive.