Homework Answers
Molar heat capacity is a measure of the amount of heat necessary to raise the temperature of one mole of a pure substance by one degree K. Specific heat capacity is a measure of the amount of heat necessary to raise the temperature of one gram of a pure substance by one degree K.
The specific heat capacity of a substance is the heat capacity of a sample of the substance divided by the mass of the sample. Informally, it is the amount of energy that must be added, in the form of heat, to one unit of mass of the substance in order to cause an increase of one unit in its temperature.
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QUESTION 3 5 points Save Answer Barium (FW = 137.3 g/mol) has a rather high molar...
QUESTION 4 0.5 points Save Answer A 6.32 g sample of ethanol (C2H5OH) is burned in...
QUESTION 4 0.5 points Save Answer A 6.32 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity, C = 5.65 kJ/°C. C2H5OH() + 3 O2(g) 2 CO2(g) + 3 H2O(g) AH®rxn = -1235 kJ If the initial temperature is 25.0°C, what is the final temperature (in °C) of the calorimeter? The molar mass of ethanol is 46.07 g/mol. Remember, in the heat equation, q = m*s*AT, heat capacity is equivalent to C= m*s, giving...
QUESTION 1 1 points Save Answer The evaporation of ethanol (molar mass = 46.07 g/mol) involves...
QUESTION 1 1 points Save Answer The evaporation of ethanol (molar mass = 46.07 g/mol) involves an enthalpy change of 0.918 kJ/g. What is the molar enthalpy of vaporization of ethanol? 0 -0.0369 kJ/mol +37.8 kJ/mol O-42.3 kJ/mol O +1.18 kJ/mol O 12.2.1.1.al Click Save and Submit to save and submit. Click Save All Answers to save all answers. Save All Answers Close Window Save and Submit
1) if 6.85 of glucose( C6H12O6, molar mass=180.2 g/mol) is dissolved in 155g of chloroform( CHCL3,molar...
1) if 6.85 of glucose( C6H12O6, molar mass=180.2 g/mol) is dissolved in 155g of chloroform( CHCL3,molar mass= 119.4 g/mol) , what is the boiling point of the solution. ( the boiling point of pure CHCl3 is 61.2 celsius, and Kb = 3.63 celsius/m for CHCl3) 2) a,) Liquid ammonia (boiling point = -33.4C) can be used as a refrigerant and heat transfer fluid. How much energy is needed to heat 25.0 g of NH3(l) from -65.0C to -12.0C? Heat of...
Question 3: (a) (6 points) We place 120.0 g of a metal at 80.00oC in 436.3...
Question 3:
(a) (6 points) We place 120.0 g of a metal at 80.00oC in
436.3 g of water at 25.00oC. The water is in a beaker
that is also at 25.00oC. The specific heat of water is
4.184 J K-1 g-1 and the heat capacity of the
beaker is 0.6666 kJ K-1. The specific heat capacity of
the metal is 0.4444 J K-1 mol-1. What is the
final temperature of the metal, the water, and the beaker?
(b) (3...
Question 3 1 pts A coffee cup calorimeter is prepared, containing 100.000 g of water (specific...
Question 3 1 pts A coffee cup calorimeter is prepared, containing 100.000 g of water (specific heat capacity 4.184 J/g K) at initial temperature 80.000 C. A salt weighing 6.303 g is quickly added. The salt has a molar mass of 321.692 g/mol. The final temperature of the solution is 43.252 C. Assume no heat loss to the surroundings. Assume the specific heat capacity of the solution is equal to that of pure water, and that the mass of the...
QUESTION 4 1 points Save Answer By how much would the temperature of 9.13 g of...
QUESTION 4 1 points Save Answer By how much would the temperature of 9.13 g of pure water increase when 0.910 kJ of heat is applied, assuming a specific heat capacity of 4.18 J/(g•°C)? Express your answer to 3 significant figures and in units of °C, but do not include units when inputting your answer. Temperature increase = ? °C Click Save and Submit to save and submit. Click Save All Answers to save all answers. Save All Answers Close...
QUESTION 4 Calculate the pH when 1.13 g of NaClO (FW = 74.44 g/mol) is added...
QUESTION 4 Calculate the pH when 1.13 g of NaClO (FW = 74.44 g/mol) is added to 32.9 mL of 0.50 M HCIO. Ignore any changes in volume. The Ka value for HCIO IS 3.0 x 10-8 1 points Save Answer
Question 22 (3 points) A 42.1 g piece of metal was heated to 95.4°C and then...
Question 22 (3 points) A 42.1 g piece of metal was heated to 95.4°C and then dropped into a beaker containing 42.0 g of water at 23.00°C. When the water and metal come to thermal equilibrium, the temperature is 32.10°C. What is the specific heat capacity of the metal? The specific heat capacity of the water is 4.184 J/(g-K) 0.387 J/(g-K) 0.600 J/(g-K) 0.488 J/(g-K) 0.720 J/(g-K) 0.980 J/(g-K)
A 92.5 g piece of aluminum (which has a molar heat capacity of 24.03]/°C-mol) is heated...
A 92.5 g piece of aluminum (which has a molar heat capacity of 24.03]/°C-mol) is heated to 624°C and dropped into a calorimeter containing water (specific heat capacity of water is 4.18 J/g°C) initially at 19.2°C. The final temperature of the water is 135.2°C. Ignoring significant figures, calculate the mass of water in the calorimeter.
Potassium nitrate, KNO,, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 25.9 g...
Potassium nitrate, KNO,, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 25.9 g of KNO, is dissolved in 319 g of water at 23.00 °C. KNO,() K+(aq) + NO (aq) The temperature of the resulting solution decreases to 20.90 °C. Assume that the resulting solution has the same specific heat as water, 4.184 J/(g: "C), and that there is negligible heat loss to the surroundings. How much heat was released by the solution? What is the enthalpy...
QUESTION 4 0.5 points Save Answer A 6.32 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity, C = 5.65 kJ/°C. C2H5OH() + 3 O2(g) 2 CO2(g) + 3 H2O(g) AH®rxn = -1235 kJ If the initial temperature is 25.0°C, what is the final temperature (in °C) of the calorimeter? The molar mass of ethanol is 46.07 g/mol. Remember, in the heat equation, q = m*s*AT, heat capacity is equivalent to C= m*s, giving...
QUESTION 1 1 points Save Answer The evaporation of ethanol (molar mass = 46.07 g/mol) involves an enthalpy change of 0.918 kJ/g. What is the molar enthalpy of vaporization of ethanol? 0 -0.0369 kJ/mol +37.8 kJ/mol O-42.3 kJ/mol O +1.18 kJ/mol O 12.2.1.1.al Click Save and Submit to save and submit. Click Save All Answers to save all answers. Save All Answers Close Window Save and Submit
Question 3:
(a) (6 points) We place 120.0 g of a metal at 80.00oC in
436.3 g of water at 25.00oC. The water is in a beaker
that is also at 25.00oC. The specific heat of water is
4.184 J K-1 g-1 and the heat capacity of the
beaker is 0.6666 kJ K-1. The specific heat capacity of
the metal is 0.4444 J K-1 mol-1. What is the
final temperature of the metal, the water, and the beaker?
(b) (3...
Question 3 1 pts A coffee cup calorimeter is prepared, containing 100.000 g of water (specific heat capacity 4.184 J/g K) at initial temperature 80.000 C. A salt weighing 6.303 g is quickly added. The salt has a molar mass of 321.692 g/mol. The final temperature of the solution is 43.252 C. Assume no heat loss to the surroundings. Assume the specific heat capacity of the solution is equal to that of pure water, and that the mass of the...
QUESTION 4 1 points Save Answer By how much would the temperature of 9.13 g of pure water increase when 0.910 kJ of heat is applied, assuming a specific heat capacity of 4.18 J/(g•°C)? Express your answer to 3 significant figures and in units of °C, but do not include units when inputting your answer. Temperature increase = ? °C Click Save and Submit to save and submit. Click Save All Answers to save all answers. Save All Answers Close...
QUESTION 4 Calculate the pH when 1.13 g of NaClO (FW = 74.44 g/mol) is added to 32.9 mL of 0.50 M HCIO. Ignore any changes in volume. The Ka value for HCIO IS 3.0 x 10-8 1 points Save Answer
Question 22 (3 points) A 42.1 g piece of metal was heated to 95.4°C and then dropped into a beaker containing 42.0 g of water at 23.00°C. When the water and metal come to thermal equilibrium, the temperature is 32.10°C. What is the specific heat capacity of the metal? The specific heat capacity of the water is 4.184 J/(g-K) 0.387 J/(g-K) 0.600 J/(g-K) 0.488 J/(g-K) 0.720 J/(g-K) 0.980 J/(g-K)
A 92.5 g piece of aluminum (which has a molar heat capacity of 24.03]/°C-mol) is heated to 624°C and dropped into a calorimeter containing water (specific heat capacity of water is 4.18 J/g°C) initially at 19.2°C. The final temperature of the water is 135.2°C. Ignoring significant figures, calculate the mass of water in the calorimeter.
Potassium nitrate, KNO,, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 25.9 g of KNO, is dissolved in 319 g of water at 23.00 °C. KNO,() K+(aq) + NO (aq) The temperature of the resulting solution decreases to 20.90 °C. Assume that the resulting solution has the same specific heat as water, 4.184 J/(g: "C), and that there is negligible heat loss to the surroundings. How much heat was released by the solution? What is the enthalpy...
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