In a chemical reaction that takes place at a fixed pressure and volume, the enthalpy change (ΔH) is –585 kJ/mol. Will this react
2 answers:
According to the sign convention, a negative Δ indicates that the reaction is exothermic, resulting in a loss of heat and a reduction in temperature.
Answer: Temperature increase
Explanation:
An endothermic reaction involves products that have higher energy than the reactants. In this kind of reaction, heat is absorbed, leading to a positive . This absorption of energy results in a decrease in the surrounding temperature.
Conversely, exothermic reactions result in products with lower energy compared to the reactants. These reactions release energy as heat, resulting in a negative . Consequently, the temperature of the surroundings increases.
Therefore, with an enthalpy change of , the temperature rises.
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Response:
Here's my calculation
Clarification:
Assume the starting concentrations of H₂ and I₂ are 0.030 and 0.015 mol·L⁻¹, respectively.
We need to determine the initial concentration of HI.
1. We will need a chemical equation with concentrations, so let's compile all the information in one location.
H₂ + I₂ ⇌ 2HI
I/mol·L⁻¹: 0.30 0.15 x
2. Calculate the concentration of HI
3. Plot the initial values
The graph below visualizes the initial concentrations as plotted on the vertical axis.
Response: k = 23045 N/m
Clarification:
To determine the spring constant, one must consider the maximum elastic potential energy that the spring can withstand. The kinetic energy of the vehicle should equal at minimum the elastic potential energy of the spring when it is fully compressed. Hence, we express it as:
(1)
The spring constant calculates to 23045 N/m