Find for this reaction as written. (Use 1.0 for the density of the solution and 4.18 as the specific heat capacity.)
When 0.129 of is combined with enough to make 53.8 of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.4 to 24.7.
You need to provide units in two or three places. You need to provide the reaction to which you refer. Where did the Zn come from?
2 places and Zn + 2HCl -- ZnCl2 + H2
Find delta Hrxn for the reaction
answer in KJ per mol
q = mass H2O x specific heat H2O x (Tfinal-Tinitial)
q/0.129 = heat/gram
(q/0.129)* atomic mass Zn = J/mol
Divide by 1000 to convert to kJ/mol
To answer this question, we need to calculate the heat released or absorbed during the reaction. We can use the formula:
q = m * C * ΔT
where:
q = heat released or absorbed (in Joules)
m = mass of the solution (in grams)
C = specific heat capacity of the solution (in J/g°C)
ΔT = change in temperature (in °C)
First, we need to find the mass of the solution. We are given that the mixture contains 0.129 g of zinc and enough HCl to make 53.8 g of solution. So, the mass of the solution is 53.8 g.
Next, we calculate the change in temperature (ΔT). The initial temperature is 22.4°C, and the final temperature is 24.7°C. The change in temperature (ΔT) is:
ΔT = final temperature - initial temperature
ΔT = 24.7°C - 22.4°C
ΔT = 2.3°C
Now, we can substitute the given values into the formula and solve for q:
q = (mass of solution) * (specific heat capacity of solution) * (change in temperature)
q = (53.8 g) * (4.18 J/g°C) * (2.3°C)
Calculating this expression will yield the heat released or absorbed during the reaction.