A student made a graph to show the chemical equilibrium position of a reaction. The student forgot to label the y-axis of the gr
aph.
What best explains the label that the student should use on the y-axis?
Reaction rate, as the rate of forward and back reaction become equal at equilibrium.
Reaction rate, as the rate of forward reaction increases and rate of backward reaction decreases with time.
Concentration, as the concentration of products decreases and that of reactants increase over time.
Concentration, as the concentrations of reactants and products remain constant after equilibrium is reached.
What best explains the label that the student should use on the y-axis?
Reaction rate, as the rate of forward and back reaction become equal at equilibrium.
Reaction rate, as the rate of forward reaction increases and rate of backward reaction decreases with time.
Concentration, as the concentration of products decreases and that of reactants increase over time.
Concentration, as the concentrations of reactants and products remain constant after equilibrium is reached.
1 answer:
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Answer:
The total heat required is 691,026.36 J
Explanation:
Latent heat is the amount of heat that a body receives or gives to produce a phase change. It is calculated as: Q = m. L
Where Q: amount of heat, m: mass and L: latent heat
On the other hand, sensible heat is the amount of heat that a body can receive or give up due to a change in temperature. Its calculation is through the expression:
Q = c * m * ΔT
where Q is the heat exchanged by a body of mass m, constituted by a substance of specific heat c and where ΔT is the change in temperature (Tfinal - Tinitial).
In this case, the total heat required is calculated as:
- Q for liquid water. This is, raise 248 g of liquid water from O to 100 Celsius. So you calculate the sensible heat of water from temperature 0 °C to 100° C
Q= c*m*ΔT
Q=103,763.2 J
- Q for phase change from liquid to steam. For this, you calculate the latent heat with the heat of vaporization being 40 and being 248 g = 13.78 moles (the molar mass of water being 18 g / mol, then
)
Q= m*L
Q=562.0862 kJ= 562,086.2 J (being 1 kJ=1,000 J)
- Q for temperature change from 100.0 ∘ C to 154 ∘ C, this is, the sensible heat of steam from 100 °C to 154°C.
Q= c*m*ΔT
Q=25,176.96 J
So, total heat= 103,763.2 J + 562,086.2 J + 25,176.96 J= 691,026.36 J
<u><em>The total heat required is 691,026.36 J</em></u>