I don't understand how you get the answer. I really don't understand any of this, how do I set it up with the numbers? once i get how to do this, then i feel i will understand how to set these up from here on out. so if you could, show all your work, thanks
(A). A reaction with a known q is performed in a bomb calorimeter and is found that 10.0 kj of heat is required to raise the temperature of the calorimeter by 2.15 degrees C. calculate the heat capacity of the calorimeter.
(B). When 1.00 g of C2H6(g) is burned in the bomb calorimeter from (A), the temperature rises from 22.00 degrees C to 33.13 degrees C. calculate q for the combustion of C2H6(g) as performed
q = Ccal x delta T
Ccal = 10,000/2.15 = 4651.2 J/K
q = [mass H2O x specific heat H2O x delta T] + [Ccal*delta T]
q = [150 x 4.184 x (33.13-22.00)] + [4651.2*(33.13-22.00)] = ??
I didn't watch my significant figures in the above. You need to take care of that after your calculation.
In #1, the heat capacity is the heat generated/degree rise in T.
In #2, the ethane burns and the water inside the calorimeter tells you how much heat is generated BECAUSE the T of the water is raised. We know the mass of the water, we know the specific heat water, and the rise in T was measured; therefore we can calculate the amount of heat generated. The heat raised the T of BOTH the water AND the calorimeter. So the total Q from burning ethane is just q from the water + q from the calorimeter.
a 225.0 gram sample of aluminum is heated and the temperature increased from 50.0 celsius to 65.0 celsius for temperature change of 15.0celsius. how many calories of heat was absorbed to produce this temperature?
Sure, I'd be happy to walk you through the process of solving these calorimetry problems step by step.
(A) To calculate the heat capacity of the calorimeter, you need to use the formula:
q = m * C * ΔT
Where:
q = heat absorbed or released by the calorimeter (in this case, 10.0 kJ)
m = mass of the substance being heated or cooled (calorimeter)
C = specific heat capacity of the substance (calorimeter)
ΔT = change in temperature (in this case, 2.15 degrees Celsius)
To solve for C, rearrange the formula:
C = q / (m * ΔT)
Now, substitute the values into the equation:
C = 10.0 kJ / (m * 2.15 °C)
Unfortunately, you haven't provided the mass (m) of the calorimeter. In order to solve for C, we need this information. Could you please provide the mass of the calorimeter?
(B) To calculate the heat released during the combustion of C2H6(g) in the calorimeter, we will use the same formula:
q = m * C * ΔT
In this case, we know that the initial temperature (Ti) is 22.00 °C, the final temperature (Tf) is 33.13 °C, and we are given the mass of C2H6(g), which is 1.00 g.
The change in temperature (ΔT) will be Tf - Ti:
ΔT = 33.13 °C - 22.00 °C = 11.13 °C
Now, we need to calculate the heat capacity of the calorimeter (C). If you have the mass of the calorimeter, you can use the value obtained from part (A). Otherwise, we can assume the heat capacity of the calorimeter (C) is the same as in part (A) and use that value.
Let's say the heat capacity of the calorimeter is C = X (where X is the value calculated in part A).
Substituting the values into the formula:
q = 1.00 g * X * 11.13 °C
Now, calculate the value of q by substituting X, the heat capacity of the calorimeter (obtained in part A), into the formula.