Question

3.An aqueous solution of Na3PO4 is heated from 24.7o C to 35.6o C. How much heat...

3.An aqueous solution of Na3PO4 is heated from 24.7o C to 35.6o C. How much heat was absorbed by the solution?

1. Consider the chemical equation below. Is the reaction endothermic or exothermic? Explain your answer. HCl(aq) + NaOH(aq) J NaCl(aq) + H2O(l) -56.13 kJ

2. In the reaction in question 1, how many kJ of energy are produced when 0.041 moles of HCl are neutralized by an excess of NaOH?

Homework Answers

Answer #1

(3) The amount of heat absorbed by the solution , Q = mcdt

Where

m = mass of the solution =

c = specific heat capacity of Na3PO4 solution = 4.057 J/g-oC

dt = change in temperature = final - initial = 35.6 - 24.7 = 10.9 oC

If we know the mass of the solution we have to fing the amount of the solution.

--------------------------------------------------------------------------------------------

(1) HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l) H = -56.13 kJ

Here the change in enthalpy is -ve that means heat is released so the reaction is exothermic reaction.

--------------------------------------------------------------------------------------------------------------------

(2) From the above balanced reaction ,

1 mole of HCl reacts with excess NaOH produces 56.13 kJ of heat

0.041 mole of HCl reacts with excess NaOH produces M kJ of heat

M = ( 0.041 x 56.13) / 1

   = 2.30 kJ

Therefore the amount of energy produced is 2.30 kJ

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
In order to verify the heat of reaction, a chemist mixes 1 liter of 1 M...
In order to verify the heat of reaction, a chemist mixes 1 liter of 1 M NaOH and 1 liter of 1 M HCl. The initial temperature of the two solutions is 25°C. The specific heat of water is 4.184 J/g°C. The enthalpy of reaction of the following is –58 kJ/mol. HCl(aq) + NaOH(aq) ® NaCl(aq) + H2O(l) A) Is this reaction exothermic or endothermic? (Will the temperature increase or decrease?) B) Considering only the specific heat of the 2...
In order to verify the heat of reaction, a chemist mixes 1 liter of 1 M...
In order to verify the heat of reaction, a chemist mixes 1 liter of 1 M NaOH and 1 liter of 1 M HCl. The initial temperature of the two solutions is 25C. The specific heat of water is 4.184 J/gC. The enthalpy of reaction of the following is –58 kJ/mol. HCl(aq) + NaOH(aq) = NaCl(aq) + H2O(l) Is this reaction exothermic or endothermic? (Will the temperature increase or decrease?) Considering only the specific heat of the 2 liters of...
When 50.00 mL of aqueous HCl was mixed with 50.00 mL of NaOH (in large excess),...
When 50.00 mL of aqueous HCl was mixed with 50.00 mL of NaOH (in large excess), the temperature of the solution increased from 25.00 °C to 30.09 °C. The reaction is NaOH(aq) + HCl(aq) ↔ NaCl(aq) + H2O(aq) -- ΔH = -57.3 kJ What was the molarity of the original HCl solution? Assume the heat capacity of the solution is the same as pure water (4.184 J/g*°C), the density of the solution is 1.00 g/mL and there is no loss...
When an aqueous solution of CaCl2 is mixed with an aqueous solution of Na3PO4, a chemical...
When an aqueous solution of CaCl2 is mixed with an aqueous solution of Na3PO4, a chemical reaction occurs resulting in the formation of Ca3(PO4)2 and NaCl. This is shown by the chemical equation: 3CaCl2 (aq) + 2Na3PO4 (aq) → Ca3(PO4)2 (s) + 6NaCl (aq) a. Describe a method for separating Ca3(PO4)2 from the product mixture. b. Once the Ca3(PO4)2 has been removed, the NaCl can be recovered. Describe a method for recovering the NaCl from the aqueous solution.
• 50.5 kJ of heat is released when 1 mole of HCl reacts with 1 mole...
• 50.5 kJ of heat is released when 1 mole of HCl reacts with 1 mole of NaOH to produce 1 mole of NaCl and 1 mole of H2O. Write a thermochemical equation for this reaction. •The equation below shows that dissolving 1 mole of NaOH in water releases 40.05 kJ of heat (q). What if there was 2 moles of NaOH, how much heat would be released (q)? NaOH(s) ​​​​Na+(aq)​+​OH-(aq)​​+​40.05 kJ • From the equation above, calculate the amount...
A) The heat of neutralization of HCl (aq) by NaOH (aq) is -55.84 kJ/mol H2O produced....
A) The heat of neutralization of HCl (aq) by NaOH (aq) is -55.84 kJ/mol H2O produced. 55 mL of 1.72 M NaOH is added to 35 mL of 2.14 M HCl. Both solutions are at 23.10°C.How many moles of water are produced by this reaction? B)The final solution resulting from the reaction in Part A has a density of 1.02 g/mL and a specific heat of 3.98 J/(g·°C). What is the final solution temperature of the solution in Part A?
Use the following information to predict ΔH for the reaction: HClO4(aq) + NaOH(aq) → NaClO4(aq) +...
Use the following information to predict ΔH for the reaction: HClO4(aq) + NaOH(aq) → NaClO4(aq) + H2O(l) Solution Mass (g) Volume (ml) Molarity (mol/L) Initial Temperature (°C) HClO4(aq) 51.99 51.98 0.500 25.42 NaOH(aq) 51.49 51.48 0.500 25.42 The HClO4(aq) solution was poured into a calorimeter with a heat capacity of 115 J/C, and allowed to sit for about 5 minutes. The NaOH(aq) solution was then added, and the temperature rose to 28.16°C. The heat absorbed by the solution/water is _______...
How do the products of these chemical equations can affect the pH of an aqueous solution?...
How do the products of these chemical equations can affect the pH of an aqueous solution? NaOH+HCl-> NaCl + H2O and CH3COOH +NaOh -> CH3COO- +Na+ +H2O
0.1 M NaOH(aq) and HCl (aq). Both solutions are assumed to have a specific heat capacity...
0.1 M NaOH(aq) and HCl (aq). Both solutions are assumed to have a specific heat capacity of 4.184 J g-1 °C-1. Calculate the ΔH of neutralization for HCl in this reaction and determine whether it’s exothermic or endothermic.
A chemical plant uses electrical energy to produce gaseous Cl2 and H2 and aqueous NaOH from...
A chemical plant uses electrical energy to produce gaseous Cl2 and H2 and aqueous NaOH from aqueous sodium chloride and water. Cl2 and NaOH are important feedstocks for producing other chemicals, while H2 is an important fuel and chemical feedstock. Consider that you are starting out with 1.5 x 105 kg of NaCl and 1.5 x 105 kg of H2O. 2 NaCl (aq) + 2 H2O (l) = Cl2 (g) + H2 (g) + 2 NaOH (aq) A. What is...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT