Directions: Please complete this worksheet on a separate piece of paper. 1. What is the specific heat of aluminum if the temperature of a 28.4 g sample of aluminum is increased by 8.1 °C when 207 J of heat is added? to mnogmaat odt selss of boboon ei groas doom wolf à (g\t 002.0)6018.S$ moil al 2. How much heat must be added to an 8.21 g sample of gold to increase its temperature by 6.2 °C? The specific heat of gold is 0.129 J/g °C. stew to g 0.20 gminiet ominolas a ni bossię nad botad ai onix to olqmse g 02.SA T to mor oitios od 0° 02.SS of 3° 00.05 mont asesooni staw odtlo suasqast of Salgmaa Istom ons o to onoqot leitini sd) auw tedWOgil OCE.O ai omis 3. How many grams of water can be heated from 20.0 °C to 75 °C using 12500.0 J?
Directions: Please complete this worksheet on a separate piece of paper. 1. What is the specific heat of aluminum if the temperature of a 28.4 g sample of aluminum is increased by 8.1 °C when 207 J of heat is added? to mnogmaat odt selss of boboon ei groas doom wolf à (g\t 002.0)6018.S$ moil al 2. How much heat must be added to an 8.21 g sample of gold to increase its temperature by 6.2 °C? The specific heat of gold is 0.129 J/g °C. stew to g 0.20 gminiet ominolas a ni bossię nad botad ai onix to olqmse g 02.SA T to mor oitios od 0° 02.SS of 3° 00.05 mont asesooni staw odtlo suasqast of Salgmaa Istom ons o to onoqot leitini sd) auw tedWOgil OCE.O ai omis 3. How many grams of water can be heated from 20.0 °C to 75 °C using 12500.0 J?
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.132QP
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![**Thermochemical Reactions and Heat Calculations**
**6. How much heat is needed when 11.8 g of iron reacts with excess oxygen according to the following equation?**
\[ 3\text{Fe}(s) + 2\text{O}_2(g) \rightarrow \text{Fe}_3\text{O}_4(g) \quad \Delta H = -1120.5 \, \text{kJ} \]
**7. What is the heat change when 13.7 g of nitrogen gas reacts with excess oxygen according to the following equation?**
\[ \text{N}_2(g) + \text{O}_2(g) \rightarrow 2\text{NO}(g) \quad \Delta H = -180 \, \text{kJ} \]
**8. How much heat is needed to react 38.2 g of bromine with excess hydrogen gas according to the following equation?**
\[ \text{H}_2(g) + \text{Br}_2(g) \rightarrow 2\text{HBr}(g) \quad \Delta H = 72.80 \, \text{kJ} \]
**9. How much heat is lost when 18.6 g of hydrogen reacts with excess oxygen according to the following equation?**
\[ 2\text{H}_2(g) + \text{O}_2(g) \rightarrow 2\text{H}_2\text{O}(l) \quad \Delta H = -571.6 \, \text{kJ} \]
**10. What is the heat change when 14.9 g of ammonia reacts with excess oxygen according to the following equation?**
\[ 4\text{NH}_3(g) + 5\text{O}_2(g) \rightarrow 4\text{NO}(g) + 6\text{H}_2\text{O}(g) \quad \Delta H = -1170 \, \text{kJ} \]
### Explanation of Graphs and Diagrams:
This document contains a series of chemical reactions along with their respective enthalpy changes (ΔH), given in kilojoules (kJ). Each reaction is presented with specific amounts of reactants to calculate the heat change for that amount of material. The ΔH value signifies whether the reaction is exothermic (negative ΔH](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7c430cc2-4097-4d45-9871-f052d1dcc428%2F89b2ff90-d87f-4be1-8f98-61c158682be9%2Fgym4a1r_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Thermochemical Reactions and Heat Calculations**
**6. How much heat is needed when 11.8 g of iron reacts with excess oxygen according to the following equation?**
\[ 3\text{Fe}(s) + 2\text{O}_2(g) \rightarrow \text{Fe}_3\text{O}_4(g) \quad \Delta H = -1120.5 \, \text{kJ} \]
**7. What is the heat change when 13.7 g of nitrogen gas reacts with excess oxygen according to the following equation?**
\[ \text{N}_2(g) + \text{O}_2(g) \rightarrow 2\text{NO}(g) \quad \Delta H = -180 \, \text{kJ} \]
**8. How much heat is needed to react 38.2 g of bromine with excess hydrogen gas according to the following equation?**
\[ \text{H}_2(g) + \text{Br}_2(g) \rightarrow 2\text{HBr}(g) \quad \Delta H = 72.80 \, \text{kJ} \]
**9. How much heat is lost when 18.6 g of hydrogen reacts with excess oxygen according to the following equation?**
\[ 2\text{H}_2(g) + \text{O}_2(g) \rightarrow 2\text{H}_2\text{O}(l) \quad \Delta H = -571.6 \, \text{kJ} \]
**10. What is the heat change when 14.9 g of ammonia reacts with excess oxygen according to the following equation?**
\[ 4\text{NH}_3(g) + 5\text{O}_2(g) \rightarrow 4\text{NO}(g) + 6\text{H}_2\text{O}(g) \quad \Delta H = -1170 \, \text{kJ} \]
### Explanation of Graphs and Diagrams:
This document contains a series of chemical reactions along with their respective enthalpy changes (ΔH), given in kilojoules (kJ). Each reaction is presented with specific amounts of reactants to calculate the heat change for that amount of material. The ΔH value signifies whether the reaction is exothermic (negative ΔH
Transcribed Image Text:**Calorimetry Review Worksheet**
**Directions:** Please complete this worksheet on a separate piece of paper.
1. **What is the specific heat of aluminum if the temperature of a 28.4 g sample of aluminum is increased by 8.1 °C when 207 J of heat is added?**
2. **How much heat must be added to an 8.21 g sample of gold to increase its temperature by 6.2 °C? The specific heat of gold is 0.129 J/g•°C.**
3. **How many grams of water can be heated from 20.0 °C to 75 °C using 12500.0 J?**
4. **What is the final temperature after 840 J is absorbed by 10.0 g of water at 25.0 °C?**
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