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Energy in Chemical Reactions II Unit Test
Energy in Chemical Reactions II Unit TestNEED HELP FAST
1. A scientist wants to perform a reaction in a vacuum chamber to control the experiment as much as possible and to prevent other variables from impacting the reaction. The scientist is trying to determine if the reaction is endothermic or exothermic and measure how much energy is absorbed or given off. Is this a valid approach? Why or why not? In three to five sentences, explain your reasoning.
2. A chemist wants to observe the following reaction:
2H2 + O2 → 2H2O
The chemist is standing inside a room with oxygen in the air and has a balloon filled with hydrogen. The chemist holds a small flame up to the hydrogen balloon. When the balloon pops, the hydrogen explodes in a ball of fire.
Based on what you know about breaking and forming bonds, explain which part of the reaction is higher in energy (i.e., does it take more energy to break the bonds of the reactants, or is more energy given off when the product bonds are formed?). Defend your answer in three to five sentences.
3. A scientist studies the bond energies of different compounds containing nitrogen (N). The scientist observes that the N–N bonds in one group of compounds have a bond energy of 209 kJ/mol, while the N–N bonds in another group of compounds have a bond energy of 418 kJ/mol. In one or two sentences, hypothesize a reason for this difference.
A scientist can validly use a vacuum chamber to determine if a reaction is exothermic or endothermic. In the hydrogen and oxygen reaction, moreenergyis released when the product bonds are formed, indicating an exothermic reaction. Differences in bond energy for N-N bonds could be due to different structures or surrounding atoms.1. Yes, performing the experiment in a vacuum chamber is a valid approach. This environment minimizes interference from other variables and allows for a more accurate measure of the reaction'sthermal properties. Whether the reaction is exothermic (releases energy) or endothermic (absorbs energy) can be determined by measuring the heat change in the chamber.2. The formation of the product bonds in the reaction 2H2 + O2 → 2H2O is likely associated with a higher energy state because when the bond forms, a large amount of energy is released, evidenced by the explosion. This strongly suggests that the reaction is exothermic—more energy is given off when product bonds are formed than it takes to break the reactants' bonds.3. The difference in bond energy for N-N bonds might be due to thecompounds' differentstructuresor different surrounding atoms in the compounds affecting the bond energy. The difference in bond energy tells us about the relative strength of the bonds — more energy suggests a stronger bond.For more such questions onenergy, click on:brainly.com/question/32125387#SPJ6...