I'm confused on number 6 on the take home test. in this problem are we going to use the heat capacity of calorimeter is 2.21kJ/c. I'm confused on how to set this problem up
1)I converted 1.000kg in to grams= 1000g
2) I used q=m*c* the change in T
1000g*(4.184J/g* C)*(295.97 K -293.37 K) =10460 J
This is where I get stuck at and i'm not sure if i set the problem up right. can you explain to me if i'm doing it right, and/or show me how to set this problem up?
2 answers
You need to pay attention to your units. The temperature for heat capacity is in given with C not K. You have to use C as temperature and not K. Also, I have no idea what the problem is asking; all I see is numbers, so I really can't check, nor can anyone else.
my professor told us to change them the temperture from C to K but I will be sure to remember that. but the problem is: A 0.3423 g sample of pentane, C5H12, was burned in a bomb calorimeter. The temperature of the calorimeter
and the 1.000 kg of water contained therein rose from 20.22°C to 22.82°C. The heat capacity of the
calorimeter is 2.21 kJ/°C. The heat capacity of water = 4.184 J/g·°C. What is the heat of combustion, in
kilojoules, per gram of pentane?
and the 1.000 kg of water contained therein rose from 20.22°C to 22.82°C. The heat capacity of the
calorimeter is 2.21 kJ/°C. The heat capacity of water = 4.184 J/g·°C. What is the heat of combustion, in
kilojoules, per gram of pentane?
1 answer