Question

What is recorded as the final temperature (in oC) on a constant pressure calorimeter if 9.377...

What is recorded as the final temperature (in oC) on a constant pressure calorimeter if 9.377 g of potassium hydroxide is dissolved in 30.431 mL of water originally at 21.094oC?

Homework Answers

Answer #1

enthalphy of solution for KOH = -57.61 KJ/mol

mass of KOH =9.377 g
Molar mass of KOH = 56.1 g/mol
number of moles of KOH = mass/ molar mass = 9.377/56.1 = 0.167 mol

Heat released = number of moles * enthalphy of solution = 0.167*57.61 = 9.6 KJ = 9600 J

Specific heat capacity of water = 4.186 J/goC
mass of water = volume * density = 30.431 mL * 1 g/mL = 30.431 g

This heat is absorbed by water
Let final temperature be T oC
Q = m*C* delta T
9600 = 30.431 * 4.186 * (T- 21.094)
T-21.094 = 75.36
T=96.45 oC
Answer: 96.45 oC

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
A student dissolves 5g of NaOH in 100mL of water at 25.0 oC in a calorimeter....
A student dissolves 5g of NaOH in 100mL of water at 25.0 oC in a calorimeter. The final temperature of the solution was found to be 35.4 oC. Assume the calorimeter constant is 92J/oC , the density of the solution is 1g/ml, and the specific heat of the solution is 4.184J/g oC. Calculate the enthalpy of solution of NaOH in kJ/mol NaOH.
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine...
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. A chunk of zinc weighing 18.01 grams and originally at 98.77 °C is dropped into an insulated cup containing 83.17 grams of water at 20.02 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.56...
1) A 32 g stainless steel ball at 110.5°C is placed in a constant pressure calorimeter...
1) A 32 g stainless steel ball at 110.5°C is placed in a constant pressure calorimeter containing 100 ml of water at 20 °C. Calculate the final temperature of water. The specific heat of the ball is 0.474 J/g°C and the specific heat of water is 4.18 J/g°C. explain plz
a reaction was conducted in an "open" (constant pressure) calorimeter. 1.00g acetic acid (HC2H3O2) is dissolved...
a reaction was conducted in an "open" (constant pressure) calorimeter. 1.00g acetic acid (HC2H3O2) is dissolved in 50.0 mL h20 (assume density 1.00g/ml specific heat 4.184j/g deg C) the temp of water was initially 25 deg C and final temp was 25.51 deg C. The process being studied is HC2H3O2(l) --> HC2H3O2 (aq). Delta H for hydration of one mole of HC2H3O2 is -7.19KJ. Calculate the Heat Capacity of calorimeter
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine...
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat capacity of a solid, or to measure the enthalpy of a solution phase reaction.   Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant.   One way to do this is to use a common metal...
two parts for one question ----------------------------------------- In the laboratory a "coffee cup" calorimeter, or constant pressure...
two parts for one question ----------------------------------------- In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant. One way to do this is...
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine...
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. A student heats 60.93 grams of gold to 98.87 °C and then drops it into a cup containing 79.68 grams of water at 24.46 °C. She measures the final temperature to be 26.11 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was...
The following data were recorded in the experiment (E106): mass of calorimeter 60g mass of calorimeter...
The following data were recorded in the experiment (E106): mass of calorimeter 60g mass of calorimeter with water 230 g mass of metal specimen 58 g initial temperature of water and calorimeter 20 ᵒC initial temperature of the metal 100 ᵒC Specific Heat Capacity of Calorimeter 0.22 cal/g. Cᵒ Final temperature of the mixture 27 ᵒC What is the specific heat capacity of the metal specimen in cal/g.ᵒC ? A .0.09 B. 0.30 C. 0.22 D. 0.03
3. A sample of metal weighing 35.5g at a temperature of 100 oC was placed in...
3. A sample of metal weighing 35.5g at a temperature of 100 oC was placed in a calorimeter containing 50 g of water at 25.0 oC. At equilibrium the temperature of water and metal was 35.5 oC. Calculate the heat capacity of the metal. . Use this value for Cp:27.65. 4. When 0.50 g of magnesium metal is placed in a calorimeter, and 100. mL of 1.0 M HCl were added the temperature of solution increased from 22.2 oC to...
A generic solid, X, has a molar mass of 67.9 g/mol. In a constant-pressure calorimeter, 16.8...
A generic solid, X, has a molar mass of 67.9 g/mol. In a constant-pressure calorimeter, 16.8 g of X is dissolved in 269 g of water at 23.00 °C. X(s) ------ X(aq) The temperature of the resulting solution rises to 26.40 °C. Assume the solution has the same specific heat as water, 4.184 J/(g·°C), and that there\'s negligible heat loss to the surroundings. 1. How much heat was absorbed by the solution? 2. What is the enthalpy of the reaction?