Question

Mass of Ca(s) 0.5 g volume of water 50.0 mL initial temp 25.6 C final temp...

Mass of Ca(s) 0.5 g
volume of water 50.0 mL
initial temp 25.6 C
final temp 48.5 C

calculate the enthalpy of dissolution of Ca in water in kJ/mol

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Given data:

The mass of Ca(s) (m) = 0.5 g, its no. of moles (n) = 0.5 g / 40 g mol-1, i.e. 0.0125 mol

The volume of water = 50 mL

Therefore, the concentration of Ca in water = (0.0125 mol / 50 L) * 1000 = 0.25 mol/L

The change in temperature (T) = 48.5 - 25.6 = 22.9 oC = (22.9 + 273.15) K = 296.05 K

The heat required for calcium (q) = (c)Ca * m * T

= 0.647 J/g•K * 0.5 g * 296.05 K

= 95.77 J

Therefore, the enthapy of dissolution of Ca in water = q/n

= 95.77 J / 0.0125 mol

= 7.66 KJ/mol

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
Mass of Ca(s) 0.5 g Volume of 1.0 M HCl 50.0 mL initial temperature 25.8 C...
Mass of Ca(s) 0.5 g Volume of 1.0 M HCl 50.0 mL initial temperature 25.8 C final temperature 45.7 C calculate the enthalpy of dissolution of Ca in acid in kJ/mol
Mass of water 200 g Volume of water 200 mL Fuel Initial mass of fuel (g)...
Mass of water 200 g Volume of water 200 mL Fuel Initial mass of fuel (g) Final mass of fuel (g) Initial temp of water (oC) Final temp of water (oC) Fuel Canister (diethylene glycol) 129.7 121.7 25 106 Tea Candle (Paraffin Wax) 12.0 11.8 25 32 Calculate the amount of energy released during the combustion of each fuel using the given equation. Show all work. Q = ΔTmcp Diethylene glycol: Tea candle: Calculate the amount of grams of each...
initial temp of solution in C 21.2 21.2 21.2 final temp of solution in C 36.4...
initial temp of solution in C 21.2 21.2 21.2 final temp of solution in C 36.4 35.2 38.7 change in temp in C 15.2 14.0 17.5 Determine Mass of solution: X X X weight of test tube with solution in g 112.24 109.57 179.48 weight of empty test tube with cap in g 63.15 63.15 63.15 mass of solution in g 49.09 46.42 116.33 Amount of heat released (J) the specific heat capacity of the solution is 5.49 J/(K x...
A solution is made by adding 0.380 g Ca(OH)2(s), 50.0 mL of 1.20 M HNO3, and...
A solution is made by adding 0.380 g Ca(OH)2(s), 50.0 mL of 1.20 M HNO3, and enough water to make a final volume of 75.0 mL. Part A Assuming that all of the solid dissolves, what is the pH of the final solution? Express your answer using three decimal places. pH =
The enthalpy change for converting 10.0g of ice at -50.0 degrees C to water at 50.0...
The enthalpy change for converting 10.0g of ice at -50.0 degrees C to water at 50.0 degrees C is ______ kJ. The specific heats of ice, water, and steam are 2.09J/g-K, 4.18J/g-K, respectively. For H2O Hfus=6.01kJ/mol and deltaHvap=40.67 kJ/mol. A)12.28 B)4.38 C)3138 D)6.47 E)9.15
When 0.500 g CaO(s) is added to 140. g H2O at 23.1 °C in a coffee...
When 0.500 g CaO(s) is added to 140. g H2O at 23.1 °C in a coffee cup calorimeter, this reaction occurs. CaO(s)+H2O(l)-->Ca(OH)2 (aq) and enthalpy = -81.9 kj/mol Calculate the final temperature of the solution. The specific heat capacity of water is 4.184
Calculate the amount of energy (in kJ) required to heat 10.0 g of water from 50.0°C...
Calculate the amount of energy (in kJ) required to heat 10.0 g of water from 50.0°C to 150.°C at constant pressure. (specific heat capacity of liquid water is 4.18 J/g⋅K; specific heat capacity of water vapor is 1.84 J/g⋅K; heat of vaporization of water is 2.260 kJ/g). (1) 16.2 kJ (2) 25.6 kJ (3) 5.4 kJ (4) 33.2 kJ (5) 1.6 kJ I know that the answer is (2) 25.6 KJ but I do not know how to get to...
A 3.98 g sample of solid NaBr (s) is dissolved in 361 mL of water in...
A 3.98 g sample of solid NaBr (s) is dissolved in 361 mL of water in a coffee cup calorimeter. Once all of the NaBr (s) is dissolved in the water, the final temperature of the solution is found to be 30.04°C. If the initial temperature of the water in the calorimeter was 21.84 °C, calculate the calorimeter constant (in J/K) for the coffee cup calorimeter. The heat of solvation of NaBr (s) is -0.60 kJ/mol.
A 5.80 g sample of solid NH4Br (s) is dissolved in 117 mL of water in...
A 5.80 g sample of solid NH4Br (s) is dissolved in 117 mL of water in a coffee cup calorimeter. Once all of the NH4Br (s) is dissolved in the water, the final temperature of the solution is found to be 6.73°C. If the initial temperature of the water in the calorimeter was 21.63 °C, calculate the calorimeter constant (in J/K) for the coffee cup calorimeter. Report your answer to three significant figures. The heat of solvation of NH4Br (s)...
A 3.56 g sample of solid NH4C2H3O2 (s) is dissolved in 418 mL of water in...
A 3.56 g sample of solid NH4C2H3O2 (s) is dissolved in 418 mL of water in a coffee cup calorimeter. Once all of the NH4C2H3O2 (s) is dissolved in the water, the final temperature of the solution is found to be 24.81°C. If the initial temperature of the water in the calorimeter was 20.81 °C, calculate the calorimeter constant (in J/K) for the coffee cup calorimeter. Report your answer to three significant figures. The heat of solvation of NH4C2H3O2 (s)...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT