Question

Please answer both questions. Thank you. 1) The temperature of a 15.0 g sample of a...

Please answer both questions. Thank you.

1) The temperature of a 15.0 g sample of a metal (specific heat 0.040 J/g⸳°C) is raised by 18.2°C. How much heat (in J) has been absorbed by the metal?

2)

  1. A calorimeter has a heat capacity of 35.45 J/°C. When 100.0 mL of a strong acid at

23.1°C is mixed with 100.0 mL of a strong base at 23.1°C, the temperature of the solution increases to 26.2°C. Assume that the density of the solution is 1.05 g/mL and its specific heat is 4.10 J/g⸳°C. Calculate:

  1. The heat absorbed by the solution

  1. The heat absorbed by the calorimeter

  1. The heat released by the reaction

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1. What is the final temperature of a solution initially at 22.0 celsius if 2.45 g...
1. What is the final temperature of a solution initially at 22.0 celsius if 2.45 g of a solid is dropped into 34.5 g of the solution resulting in the reaction between the two that absorbs 1350 J of heat? 2. If a 31.25g piece of an unknown metal at 25 Celsius was added to 25.0 g of water at 100.0Celsius and the two equilibrated at 95.2 Celsius , what is the specific heat capacity of the metal? 3. In...
A 6.40 g sample of iron (specific heat capacity = 0.451 J/g*C) is placed in a...
A 6.40 g sample of iron (specific heat capacity = 0.451 J/g*C) is placed in a boiling water bath until the temperature of the metal is 100.0*C. The metal is quickly transferred to 119.0g of water at 25.0*C in a calorimeter (specific heat capacity of water = 4.18 J/g*C). Determine the final temperature of the water in the calorimeter (3 significant figures).
A 6.40 g sample of iron (specific heat capacity =0.451 J/g*C) is placed in a boiling...
A 6.40 g sample of iron (specific heat capacity =0.451 J/g*C) is placed in a boiling water bath until the temperature of the metal is 100.0*C. The metal is quickly transferred to 119.0g of water at 25.0*C in a calorimeter (specific heat capacity of water = 4.18 J/g*C). Determine the final temperature of the water in the calorimeter (3 significant figures).
25.0 mL of a 0.50 M solution of acid HA was combined with 25.0 mL of...
25.0 mL of a 0.50 M solution of acid HA was combined with 25.0 mL of a 0.50 solution of base MOH in a calorimeter with a calorimeter constant of 13.5 J/C. The initial temperature of the solution was 23.3 C and the maximum temperature was 34.7 C. The resulting solution had a specific heat capacity of 3.92 J/g·C and a density of 1.04 g/mL. Calculate each of the following a) The mass of the resulting solution. b) The heat...
100.0 g of an aqueous solution containing lead nitrate and 100.0 g of an aqueous solution...
100.0 g of an aqueous solution containing lead nitrate and 100.0 g of an aqueous solution containing sodium iodide (both solutions at 22.6 C), are mixed in a calorimeterwith a heat capacity of 472 J/C.; thereactants undergo a metathesis reaction that raises thetemperature of the mixture to 24.2 C. Calculate the amount of heat generated by the reaction, correcting for the heat absorbed by the calorimeter and assuming that the specific heat of the reaction solution is the same as...
1. The specific heat of iron metal is 0.450 J/g⋅K. How many J of heat are...
1. The specific heat of iron metal is 0.450 J/g⋅K. How many J of heat are necessary to raise the temperature of a 1.05 −kg block of iron from 28.0 ∘Cto 85.0 ∘C? 2. A 1.80-g sample of phenol (C6H5OH) was burned in a bomb calorimeter whose total heat capacity is 11.66 kJ/∘C. The temperature of the calorimeter plus contents increased from 21.36∘Cto 26.37∘C. A. Write a balanced chemical equation for the bomb calorimeter reaction. B. What is the heat...
PLEASE SHOW ALL WORK! 1) 65 g of ice at -17°C is mixed with 256 g...
PLEASE SHOW ALL WORK! 1) 65 g of ice at -17°C is mixed with 256 g of water at 29.2°C. Calculate the final temperature of the mixture. Assume that no energy in the form of heat is transferred to the environment. (Heat of fusion = 333 J/g; specific heat capacities: ice = 2.06 J/g x K, liquid water = 4.184 J/g x K) 2) In the reaction of barium chloride with potassium phosphate, barium phosphate and potassium chloride are produced....
A calorimeter contains 33.0 mL of water at 15.0 ∘C . When 2.10 g of X...
A calorimeter contains 33.0 mL of water at 15.0 ∘C . When 2.10 g of X (a substance with a molar mass of 46.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 28.0 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...
Assume you use calorimetry to calculate the specific heat capacity of a 125.24 g piece of...
Assume you use calorimetry to calculate the specific heat capacity of a 125.24 g piece of unknown metal. You intially heat the metal to 100.0 °C in boiling water. You then drop the chunk of metal into a calorimeter containing 45.22 g of water at 21.6 °C. After closing and stiring the calorimeter thoroughly, the metal and water both come to equilibrium at a temperature of 28.3 °C. 1. What is the temperature change of the water? 6.7 °C 21.6...
A calorimeter contains 35.0 mL of water at 15.0 ∘C . When 1.70 g of X...
A calorimeter contains 35.0 mL of water at 15.0 ∘C . When 1.70 g of X (a substance with a molar mass of 76.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 25.0 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT