### Calorimetry Problem: Heat of Combustion Calculation**Scenario:**When 0.0801 mol of an unknown hydrocarbon is burned in a bomb calorimeter, the calorimeter's temperature increases by 2.19°C. Given that the heat capacity of the bomb calorimeter is 1.229 kJ/°C, calculate the heat of combustion for the unknown hydrocarbon in kJ/mol.**Solution Steps:**1. **Determine Heat Absorbed by Calorimeter:** - Formula: \( q = C \times \Delta T \) - Where \( q \) is the heat absorbed, \( C \) is the heat capacity, and \( \Delta T \) is the change in temperature. - Substitute the values: \( q = 1.229 \, \text{kJ/°C} \times 2.19 \, \text{°C} \) - Calculate \( q \).2. **Calculate Heat of Combustion:** - Since the reaction involved 0.0801 mol of the hydrocarbon, find the heat of combustion (in kJ/mol) using the formula: - \( \text{Heat of Combustion} = \frac{q}{\text{moles of hydrocarbon}} \)3. **Final Calculation:** - Use the values derived to find the heat of combustion per mole.This setup involves a numerical keypad for input, allowing direct calculation of results, enhancing the interactive learning experience for students.**Note:** Exact calculations are omitted as it requires step-by-step computational work.

Answered: Image /qna-images/answer/5ac4ed7d-8429-40d1-aa4a-14638ad01484.jpg

Question 2 of 8 Submit When 0.0801 mol of an unknown hydrocarbon is burned in a bomb calorimeter, the calorimeter increases in temperature by 2.19°C. If the heat capacity of the bomb calorimeter is 1.229 kJ/°C, what is the heat of combustion for the unknown hydrocarbon, in kJ/mol? kJ/mol 1 2 3 4 6. C 7 8 9. +/- x 100 II <

Question 2 of 8 Submit When 0.0801 mol of an unknown hydrocarbon is burned in a bomb calorimeter, the calorimeter increases in temperature by 2.19°C. If the heat capacity of the bomb calorimeter is 1.229 kJ/°C, what is the heat of combustion for the unknown hydrocarbon, in kJ/mol? kJ/mol 1 2 3 4 6. C 7 8 9. +/- x 100 II <

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

3 aluempts let Check my work Enter your answer in the provided box. Hi A 32.0-g sample of an unknown metal at 99°C was placed in a constant-pressure calorimeter containing 75.0 g of water at 24.0°C. The final temperature of the system was found to be 28.4°C. Calculate the specific heat of the metal. (The heat capacity of the calorimeter is 14.4 J/°C.) Solu Guided S J/g °C < Prev 14 of 26
1
What is the answer by steps please
Il Metro by T-Mobile 1:06 AM n 24% Question 15 of 35 Submit Specific Heat Capacity J/(g•°C) Metal Aluminum 0.90 Сopper 0.38 Iron 0.45 Magnesium 1.00 Silver 0.23 Tin 0.32 Titanium 0.52 A) Fe B) Sn C) Ag D) Cu Tap here or pull up for additional resources
Please answer both the parts of question otherwise I'll downvote
SUBJECT : GENERAL CHEMISTRY 2 TOPIC : HEAT AND CALORIMETRY
H8. A student combined 107.5 mL of 0.2400 M HCl and 127.9 mL of 0.3650 M NaOH in a calorimeter of negligible heat capacity . The reactants were initially at 27.1 degrees Celsius. Determine the final temperature this mixture should reach in degrees Celsius (oC), given that the heat of neutralization of this reaction is -56.2 kJ/1 mol water, the specific heat capacity of water is 4.184 J/(g.oC) and assuming that the density of all the solutions is 1.00 g/mL (Hint: The reaction between an acid and a base produces a salt and water)
calculating heat of combustion of quinone
Question 17 of 35 Submit When 1.151 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose? kJ/mol 1 3 4 C 7 +/- x 10 0 Tap here or pull up for additional resources LO 00
Isooctane is a primary component of gasoline and gives gasoline its octane rating. Burning 1.00 ml of isooctane (d= 0.0688 g/ml releases 33.0 kj of heat when 10.00 ml of isooctane is burned in a bomb calorimeter, the temperature in the bomb rises from 23.2 celsius to 66.5 celsius. what is the heat capacity of the bomb calorimeter?
Answer the attached photo.
Hello! I need answers in these three questions. Would really help a lot!