A reaction occurs in a calorimeter, resulting in the starting and final temperatures shown below. What can you say about the rea
ction and the enthalpy change (ΔH) during the reaction?
ReactionEnergyAQ1
A. The reaction is endothermic and ΔH is positive.
B. The reaction is endothermic and ΔH is negative.
C. The reaction is exothermic and ΔH is positive.
D. The reaction is exothermic and ΔH is negative.
ReactionEnergyAQ1
A. The reaction is endothermic and ΔH is positive.
B. The reaction is endothermic and ΔH is negative.
C. The reaction is exothermic and ΔH is positive.
D. The reaction is exothermic and ΔH is negative.
1 answer:
Answer:
The reaction is exothermic and ΔH is negative
Explanation:
An exothermic reaction is a chemical reaction that releases energy in the form of heat. It is the opposite of an endothermic reaction in which energy is absorbed. It is expressed in a general thermochemical equation: reactants → products + energy.
We can know that a reaction is exothermic by observing the calorimeter to know if there is an increase in temperature. Remember that an exothermic reaction leads to evolution of heat. This is observed physically as a rise in temperature.
The calorimeter initially read 21.0 and finally read 38.8 at the end of the reaction. This implies that heat was given out in the process. The reaction is exothermic and ∆H is negative.
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Answer:
Explanation:
Hello there!
In this case, since the equation for the calculation of dilutions is:
Whereas M is the molarity and V the volume, because the final concentration is lower than the initial. Thus, since we are asked to calculate the final volume, we solve for V2 as follows:
Best regards!
Answer:
19.27
Explanation:
Some values are corrected from correct source.Thus,
Moles of SO₂ = 8.19x10⁻² moles
Moles of O₂ = 8.10x10⁻² moles
Volume = 1 L
Concentration of SO₂ = 8.19x10² M
Concentration of O₂ = 8.10x10 M
Considering the ICE table for the equilibrium as:
2SO₂ (g) + O₂ (g) ⇔ 2SO₃ (g)
t = o 8.19x10⁻² 8.19x10⁻²
t = eq -2x -x 2x
--------------------------------------------- --------------------------
neq: 8.19x10⁻² -2x 8.19x10⁻² -x 2x
Given:
Equilibrium concentration of O₂ = 5.98x10⁻² M = 8.19x10⁻² -x
Thus, x = 0.0212 M
[SO₂] = 8.19x10⁻² - 2*0.0212 = 0.0395 M
[SO₃] = 2*0.0212 = 0.0424 M
The expression for the equilibrium constant is:
K = 19.27
<h2>Answer:</h2>
6.67moles
<h2>Explanations:</h2>
Given the balanced chemical reaction between hydrogen and oxygen expressed as:
First, you need to calculate the moles of water produced.
Based on stochiometry, 2 moles of hydrogen produces 2 moles of water, hence the moles of hydrogen that will be needed to produce 120g of water is 6.67moles