Question

When 2.50 g of Ba(s) is added to 100.00 g of water in a container open...

When 2.50 g of Ba(s) is added to 100.00 g of water in a container open to the atmosphere, the reaction shown below occurs and the temperature of the resulting solution rises from 22.00°C to 40.32°C. If the specific heat of the solution is 4.18 J/(g • °C), calculate ΔH for the reaction, as written. Ba(s) + 2 H2O(l) → Ba(OH)2(aq) + H2(g) ΔH = ?

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
When 4.50 g of Ba(s) is added to 100.00 g of water in a container open...
When 4.50 g of Ba(s) is added to 100.00 g of water in a container open to the atmosphere, the reaction shown below occurs and the temperature of the resulting solution rises from 22.00°C to 54.35°C. If the specific heat of the solution is 4.18 J/(g • °C), calculate ΔH for the reaction, as written. Ba(s) + 2 H2O(l) → Ba(OH)2(aq) + H2(g) ΔH = ? When 4.50 g of Ba(s) is added to 100.00 g of water in a...
A. Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide according to the...
A. Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide according to the chemical equation shown below. When 0.020 mol of Na is added to 100.00 g of water, the temperature of the resulting solution rises from 25.00°C to 33.60°C. If the specific heat of the solution is 4.18 J/(g • °C), calculate ΔH for the reaction, as written. 2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g) ΔH= ? Sodium metal reacts with water to...
1. The addition of 3.27 g of Ba(OH)2 · 8 H2O to a solution of 1.14...
1. The addition of 3.27 g of Ba(OH)2 · 8 H2O to a solution of 1.14 g of NH4SCN in 175 g of water in a calorimeter caused the temperature to fall by 4.9°C. Assuming the specific heat of the solution and products is 4.20 J/g·°C, calculate the approximate amount of heat (in J) absorbed by the reaction, which can be represented by the following equation. Ba(OH)2 · 8 H2O(s) + 2 NH4SCN(aq) → Ba(SCN)2(aq) + 2 NH3(aq) + 10...
In a constant-pressure calorimeter, 70.0 mL of 0.340 M Ba(OH)2 was added to 70.0 mL of...
In a constant-pressure calorimeter, 70.0 mL of 0.340 M Ba(OH)2 was added to 70.0 mL of 0.680 M HCl. The reaction caused the temperature of the solution to rise from 22.00 °C to 26.63 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/g·K, respectively), what is ΔH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes.
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...
A calorimeter contains 30.0 mL of water at 11.5 ∘C . When 2.10 g of X...
A calorimeter contains 30.0 mL of water at 11.5 ∘C . When 2.10 g of X (a substance with a molar mass of 42.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 30.0 ∘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...
A calorimeter contains 17.0 mL of water at 11.5 ∘C . When 1.60 g of X...
A calorimeter contains 17.0 mL of water at 11.5 ∘C . When 1.60 g of X (a substance with a molar mass of 79.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 30.0 ∘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...
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...
A calorimeter contains 35.0 mL of water at 11.5 ∘C . When 1.30 g of X...
A calorimeter contains 35.0 mL of water at 11.5 ∘C . When 1.30 g of X (a substance with a molar mass of 66.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 29.5 ∘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...
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
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT