Question

In: Chemistry

2. A 155 g sample of iron metal at 120.0C is placed into 250.0 g of...

2. A 155 g sample of iron metal at 120.0C is placed into 250.0 g of water at 20.0 °C in a calorimeter. When the system reaches thermal equilibrium, the temperature of the water in the calorimeter is 30.8C. Assume the calorimeter is perfectly insulated. What is the specific heat of iron? What is the amount of heat for 80.0 g piece of iron?

Solutions

Expert Solution

Heat lose of Iron                            =      heat gain of water

mct                                           =         mct

155*C*(120-30.8)                       =         250*4.18*(30.8-20)

155*C*89.2                                =         250*4.18*10.8

13826*C                                  =         11286

            C                                  =       11286/13826 = 0.816j-C0/g

What is the amount of heat for 80.0 g piece of iron

q    = mCt

      = 80*0.816*(120-30.8)

      = 80*0.816*89.2

    = 5822.976joule


Related Solutions

b) A 50.53 g sample of a metal at 290.00 C is placed in a calorimeter...
b) A 50.53 g sample of a metal at 290.00 C is placed in a calorimeter containing 150.00 g of water at 20.00 C. The temperature stopped changing at 29.42 C. What is the specific heat of the metal? What is the identity of the metal? c) A 150.0 g sample of copper at 75.00 C is added to 150.00 g of water initially at 23.00 C Assuming that all of the heat lost by the copper is absorbed by...
A 10.540 g iron bar is warmed to 250.0 c and then plunged into 5000 ml...
A 10.540 g iron bar is warmed to 250.0 c and then plunged into 5000 ml of water at 25 c. After the iron cools the final temp of the iron and water is 27.5 C. calculate the specific heat capacity and the molar heat capacity of iron.
25. Aluminum metal shavings (10.0 g) are placed in 120.0 mL of 6.00 M hydrochloric acid....
25. Aluminum metal shavings (10.0 g) are placed in 120.0 mL of 6.00 M hydrochloric acid. What is the maximum mass of hydrogen that can be produced (in grams)? 2Al(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2(g) a. 11.5 g          b.   0.0505 g                         c. 4.76 g                      d. 0.727 g       e. 31.8 g          f.   1.42 g                     g. 3.67 g                      h.   5.13 g 26. What is the maximum number of grams of ammonia, NH3, which can be obtained...
25. Aluminum metal shavings (10.0 g) are placed in 120.0 mL of 6.00 M hydrochloric acid....
25. Aluminum metal shavings (10.0 g) are placed in 120.0 mL of 6.00 M hydrochloric acid. What is the maximum mass of hydrogen that can be produced (in grams)? 2Al(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2(g) a. 11.5 g          b.   0.0505 g                         c. 4.76 g                      d. 0.727 g       e. 31.8 g          f.   1.42 g                     g. 3.67 g                      h.   5.13 g 26. What is the maximum number of grams of ammonia, NH3, which can be obtained...
1. A 48.0−g sample of an unknown metal at 99°C was placed in a constant-pressure calorimeter...
1. A 48.0−g sample of an unknown metal at 99°C was placed in a constant-pressure calorimeter containing 70.0 g of water at 24.0°C. The final temperature of the system was found to be 28.4°C. Calculate the specific heat of the metal. (The heat capacity of the calorimeter is 10.4 J/°C.) 2.A balloon 19.0 m in diameter is inflated with helium at 23°C. Calculate the work done (in kJ) during the inflation process if the atmospheric pressure is 97.7 kPa. 3.Ice...
A 15.0g sample of an unknown metal at 85.0*C was placed in 60.0g of water at...
A 15.0g sample of an unknown metal at 85.0*C was placed in 60.0g of water at 20.0*C. the final temperature of the metal and water was 25.8*C. calculate the metal's specific heat (please show the work) how much heat in calories and joules is required to raise the temperature of 75.0g of a substance (specific heat is 1.80cal/g x *C) from 25.0*C to 95.0*C? please show the work. thank you
A 1.0 gram sample of an unknown metal was heated to 75 C, and then placed...
A 1.0 gram sample of an unknown metal was heated to 75 C, and then placed in a calorimeter filled with 100mL of water that had an initial temperature of 26 C. Once the system was allowed to reach thermal equilibrium the temperature of the water was 31 C. what is the specific heat capacity of the metal?
A 250.0 mL sample of spring water was treated to convert any iron present to Fe2+....
A 250.0 mL sample of spring water was treated to convert any iron present to Fe2+. Addition of 24.00 mL of 0.002543 M K2Cr2O7 resulted in the reaction 6Fe2+ + Cr2O72- + 14H+ ---> 6Fe3+ + 2Cr3+ + 7H2O The excess K2Cr2O7 was back titrated with 8.02 mL of 0.00971 M Fe2+ solution. Calculate the concentration of iron in the sample in ppm.
What is the vapor pressure of a 34.6 g sample of ethanol (C2H5OH) in 120.0 mL...
What is the vapor pressure of a 34.6 g sample of ethanol (C2H5OH) in 120.0 mL of water if the vapor pressure of water is 24.4 mmHg and the density is 0.9945 g/mL? Answer choices: A. 0.751 atm B. 0.0288 atm C. 21.9 atm D. 6.99 atm
A 91.70 g sample of metal was heated in a boiling water bath at 99.4 °C....
A 91.70 g sample of metal was heated in a boiling water bath at 99.4 °C. The hot metal was then placed in a calorimeter, with heat capacity 39 J/K containing 45.0 g of water. Analysis of the thermogram showed the initial temperature to be 21.1°C, the final temperature to be 42.3°C. 4.91 g of LiCl was dissolved in 50.0 mL of water in the same calorimeter as in problem (above) 1. Analysis of the thermogram showed the initial temperature...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT