ZuoTi.Pro
Question

When a 2.00g (0.0200 mol) KHCO3 was mixed with 30.0 mL of approximately 2M HCl, the...

When a 2.00g (0.0200 mol) KHCO3 was mixed with 30.0 mL of approximately 2M HCl, the temperature fall by 3.7oC

Calculate the enthalpy change of this reaction per mole of KHCO3.

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

Solution-
The equation can be written as
K2CO3 + 2HCl → 2KCl + H2O + CO2
As we know that
Q = msΔT
we know that
Mass = Volume*Density
Putting the values in the equation
= 30ml*1.00g/ml
= 30g
Given
Mass = 30g
Specific heat of mixture = 4.184 J/goC
ΔT = 3.70C
substute these value we get
Q = (30g)(4.184J/goC)(3.70C)
= 464.424 J
This is for 0.02 mol of K2CO3 .
The amount of heat liberated per one mole of K2CO3= 464.424 J * 1 mol / 0.02 mol
  

= 23221.2J
As the temperature of mixture falls it indicates that the heat is decrease, Therefore the ΔH must have +vesign.


=>ΔH = 23221.2 J

0 0
Add a comment
Know the answer?
Add Answer to:
When a 2.00g (0.0200 mol) KHCO3 was mixed with 30.0 mL of approximately 2M HCl, the...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • 2. When 2.76 g (0.0200 mol) of K2CO3 was mixed with 30.0 ml of approximately 2M...

    2. When 2.76 g (0.0200 mol) of K2CO3 was mixed with 30.0 ml of approximately 2M HCl, the temperature rose by 5.2°C. a) write a balanced equation for this reaction: b) Calculate the enthalpy change of this reaction per mole of potassium carbonate. Assume that the specific heat of the final mixture is 4.184 J/g°C, and that its density is 1.00 g/ml. 3. When 2.00 g (0.0200 mole) of potassium hydrogen carbonate (KHCO3) is mixed with 30.0 ml of the...

  • When a 2.76g (0.0200 mol) K2CO3 was mixed with 30.0 mL of approximately 2M HCl, the...

    When a 2.76g (0.0200 mol) K2CO3 was mixed with 30.0 mL of approximately 2M HCl, the temperature rose by 5.2oC Calculate the enthalpy change of this reaction per mole of K2CO3. Assume that the specific heat of tyhe final mixture is 4.184 J/goC and that its density is 1.00g/mL Please explain how do you do the enthalpy change part and how do you use the formula to find the change.

  • skip (a): the balancing part! just solve (b) 2. When 2.76 g (0.0200 mol) of K,CO,...

    skip (a): the balancing part! just solve (b) 2. When 2.76 g (0.0200 mol) of K,CO, was mixed with 30.0 ml of approximately 2M HCI, the temperature rose by 5.2 °C. (a) Write a balanced equation for this reaction. (b) Calculate the enthalpy change (AH) of this reaction per mole of potassium carbonate. Assume that the specific heat of the final mixture is 4.184 J/gºC, and that its density is 1.00 g/mL.

  • When 50.0 mL of 1.00 M HCl and 50.0 mL of 1.00 M NaOH are mixed...

    When 50.0 mL of 1.00 M HCl and 50.0 mL of 1.00 M NaOH are mixed in a constant-pressure calorimeter, the temperature of the solution increases from 21.0°C to 27.5°C. Calculate the enthalpy change of the reaction per mole of HCl assuming the solution has a total volume of 100.0 mL and a density of 1.000 g/mL. The specific heat of water is 4.184 J/q°C Asoln = 2720

  • When a chemist mixed 3.33 g of LiOH and 255 mL of 0.62 M HCl in...

    When a chemist mixed 3.33 g of LiOH and 255 mL of 0.62 M HCl in a constant-pressure calorimeter, the final temperature of the mixture was 23.4°C. Both the HCl and LiOH had the same initial temperature, 20.4°C. The equation for this neutralization reaction is: LiOH(s) + HCl(aq) → LiCl(aq) + H2O(l). Given that the density of each solution is 1.00 g/mL and the specific heat of the final solution is 4.1801 J/g·K, calculate the enthalpy change for this reaction...

  • 2. A 49.45 mL volume of 1.00 M HCl was mixed with 49.14 mL of 2.00...

    2. A 49.45 mL volume of 1.00 M HCl was mixed with 49.14 mL of 2.00 M NaOH in a coffee cup calorimeter (with calorimeter constant = 25.1 J/°C) at 21.34 °C. The final temperature of the aqueous solution after the reaction was 29.37 °C. Assuming that them heat capacity of the solution is 4.18 J/g/°C, calculate the following: e. The enthalpy change (∆H) for the neutralization in kJ/mol HCl ( this should be a negative number) e. The enthalpy...

  • HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(1) 100.0 mL of 0.500 M HCl is mixed with...

    HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(1) 100.0 mL of 0.500 M HCl is mixed with 300.0 mL of 0.100 M NaOH in a coffee cup calorimeter. Assuming the temperature of the solution was initially 25.0 °C, and the final temperature of the solution was 26.7 °C, calculate the enthalpy of this reaction per mole of HCl. Assume the density of the water and acid and base solutions are all 1.00 g/mL.

  • When 25.0 mL of 0.700 mol/L NaOH was mixed in a calorimeter with 25.0 mL of...

    When 25.0 mL of 0.700 mol/L NaOH was mixed in a calorimeter with 25.0 mL of 0.700 mol/L HCl, both initially at 20.0 °C, the temperature increased to 22.1 °C. The heat capacity of the calorimeter is 279 J/°C. What is the enthalpy of neutralization in kJ/ mole of HCl? Since the solutions are mostly water, the solutions are assumed to have a density of 1.0 g/mL and a specific heat of 4.18 J/g°C.  Select one: a. −1020 b. -58.6  c. −5856 d. 58.6

  • A 48.53 mL volume of 1.00 M HCl was mixed with 47.70 mL of 2.00 M...

    A 48.53 mL volume of 1.00 M HCl was mixed with 47.70 mL of 2.00 M NaOH in a coffee cup calorimeter (with calorimeter constant = 26.0 J/°C) at 21.43 °C. The final temperature of the aqueous solution after the reaction was 29.71 °C. Assuming that them heat capacity of the solution is 4.18 J/g/°C, calculate the following: a. The total mass of aqueous solution inside the calorimeter (dsoln = 1.00 g/mL) g b. The change in temperature (∆T) of...

  • 2. A 49.21 mL volume of 1.00 M HCl was mixed with 48.05 mL of 2.00...

    2. A 49.21 mL volume of 1.00 M HCl was mixed with 48.05 mL of 2.00 M NaOH in a coffee cup calorimeter (with calorimeter constant = 25.6 J/°C) at 20.32 °C. The final temperature of the aqueous solution after the reaction was 29.83 °C. Assuming that them heat capacity of the solution is 4.18 J/g/°C, calculate the following: a. The total mass of aqueous solution inside the calorimeter (dsoln = 1.00 g/mL) g correct 1/1 b. The change in...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT