Computation of Calories per Mass of Food Mass of can (g) 12.63 Mass of can and water (g) 111.47 Initial mass of food sample (g) 1.85 Final mass of food sample (g) 0.44 Initial temperature of water (°C) 23.05 Final temperature of water (°C) 25.17 Mass of water (g) Temperature change of water (°C). Do not include a negative sign. Heat gained by water (cal). Do not include a negative sign. Heat gained by water (kcal). Do not include a negative sign. Heat lost by food (cal). Do not include a negative sign.

Computation of Calories per Mass of Food Mass of can (g) 12.63 Mass of can and water (g) 111.47 Initial mass of food sample (g) 1.85 Final mass of food sample (g) 0.44 Initial temperature of water (°C) 23.05 Final temperature of water (°C) 25.17 Mass of water (g) Temperature change of water (°C). Do not include a negative sign. Heat gained by water (cal). Do not include a negative sign. Heat gained by water (kcal). Do not include a negative sign. Heat lost by food (cal). Do not include a negative sign.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Use the following information to answer the next question. Calcium carbonate as many uses including in the oil industry it is as a weighting material to increase the density of drilling fluids. Calcium carbonate decomposes according to the following reaction equation: CaCO3(s)→ CO₂(g) + CaO(s) The standard enthalpy of reaction for the reaction shown above is + + kJ. Record your 4-digit answer. Include sign; do not include units.
A 80.8 g chunk of granite (specific heat: 0.79 J/g°C) is heated to 225.7 °C and dropped into a beaker containing 150.0 g of methanol (specific heat: 2.549 J/g°C) at 27.1 °C.What will be the final temperature of the system after it reaches thermal equilibrium?
when 11.0 g naoh is dissolved in 100.0 g of water in a coffee-cup calorimeter, the temperature rises from 25.22c to 48.00c. what is the enthalpy change?
i need help answering this question
When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
The table lists the specific heat capacities of select substances. Substance Specific heat capacity (J/g °C) lead 0.128 silver 0.235 copper 0.385 iron 0.449 aluminum 0.903 water 4.184 An unknown substance has a mass of 19.5 g.19.5 g. The temperature of the substance increases by 16.1 ∘C16.1⁢ ∘C when 73.8 J73.8 J of heat is added to the substance. What is the most likely identity of the substance?
classify each of the following as exothermic or endothermic and give the change in heat, C3H8(g) +5O2(g) --change--> 3CO2(g) +4H2O(g) +2220 kj 2Na(s) +Cl2(g)---> 2NaCl(s)+819 kj PCl5(g) +67kj ---> PCl3(g) +Cl2(g)
A 35.0 gram object has a specific heat of 0.832 Joules/gram °C. It gained 2095 Joules of heat from the surroundings. If it had started at 25.0 °C, what was the temperature of the object after it gained the heat from the surroundings? O 25.0 degrees Celsius O 3640 degrees Celsius O 71.9 degrees Celsius O 196.9 degrees Celsius O 1.74 degrees Celsius O 53.1 degrees Celsius O 96.9 degrees Celsius
IT The temperature of a sample of aluminum increased by 24.6 °C when 255 J of heat was applied. Substance Specific heat J/(g lead 0.128 What is the mass of the sample? silver 0.235 copper 0.385 iron 0.449 aluminum 0.903 m =
You are given 50g of an unknown metal. You apply 6000J of energy to the metal, raising its temperature from 25°C to 955°C. What is the specific heat of the metal? ______ J/g°C After calculating the specific heat in J/g°C, What is the identity of the metal? Metal Specific Heat (J/g°C) Metal Specific Heat (J/g°C) Magnesium 1.02 Silver 0.24 Aluminum 0.90 Tin 0.21 Potassium 0.75 Lead 0.16 Calcium 0.65 Gold 0.129
A 6.55 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. Wht is the change in teperature in celcios inside the calometer? was the dissolution process endothermic or exothermic? how much heat, in J, was hained b the solution? assume the specific heat of the solution is the same as water, 4.184 J/g. celcius
A 151.6-g sample of a metal at 74.7°C is added to 151.6 g at 15.9°C. The temperature of the water rises to 18.2°C. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the water. The specific heat capacity of water is 4.18 J/°C ⋅ g. Specific heat capacity = ________J/°C ⋅ g