I’m stupid I can’t even answer this
Answer:
Explanation:
Hello!
In this case, since the combustion analysis provides us the yielded mass of both water and carbon dioxide, as the sources of hydrogen and carbon in the hydrocarbon, we are able to compute the moles of each via the following mole-mass relationships:
Now, we divide those moles by the fewest ones (those of carbon) in order to compute their subscripts in the empirical formula:
However we need whole numbers, that is why we multiply each subscript by 4 to get 4 for carbon and 5.08 ≅ 5 for hydrogen:
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The correct answer is option B. i.e. E°cell > 0 = spontaneous reaction.
The spontaneous reactions always have positive voltage and the energy released in the reaction is used up to do work.
Answer:
Increasing pressure shifts rxn right (lower molar volume side of equation).
Explanation:
In general, if a stress is applied to a gas phase reaction, the reaction will shift away from the applied stress and establish a new equilibrium for the given reaction. The applied stress factors include ...
changes in masses of reactant or product,
changes in applied temperature values, and/or
changes in applied pressure values for a reaction confined in a reaction vessel.
For this problem, if pressure is increased on the reaction N₂(g) + 3H₂(g) ⇄ 2NH₃(g), the reaction will shift away from the applied stress, that is, in the direction of the product side of the reaction in order to relieve the applied stress as there are fewer number of moles of gas on the product side of the equation.
Answer: true
Explanation:
In chemical reactions, an energy barrier exists between reactants and products. The magnitude of this energy barrier determines the rate of reaction. A lesser energy barrier implies that reactants are converted to products faster since the energy required is not too much. On the other hand, a large energy difference between reactants and products will lead to a slow reaction with very poor yield of products if any.