Exercise The overall reaction in a commercial heat pack can be represented as 4Fe(s) + 30, (g)→ 2Fe,O, (s) AH = -1652 kJ How much heat is released when 4.00 moles of iron are reacted with excess 0,? How much heat is released when 1.00 mole of Fe,03 is produced? 4Fe(s) + 30, (g)→ 2Fe,O, (s) AH = -1652 kJ CLC CHM121 AUDI Page 7 Chapter 6: Thermochemistry How much heat is released when 1.00 g iron is reacted with excess O,?
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- 59. When 24.0 g of carbon and 10.0 g of hydrogen are placed in a calorimeter and reacted according to the equation 3 C(s) + 4 H2(g) → C3H8(g) + 103.8 kJ, the maximum amount of heat liberated by this reaction is? (hint: limiting reagent) Answer: 69.1 kJneed it fast!!!!!!! Gaseous hydrogen and liquid bromine combine in the reaction below to form hydrogen bromide (HBr) in its gaseous state: H2(g) + Br2(l) --> 2 HBr(g) If ∆Ho for this reaction is -72.4 kJ, what is the standard enthalpy of formation, Hfo, for gaseous hydrogen bromide, in kJ? answer:_____________________What I Have Learned Activity 3.4.3. Solve me! 1. Calculate the heat of hydrogena tion of ethane, C₂H, given the followi ng thermochemical equations 2 C(graphite) 3 H₂ (g) C₂He (g) 2C (graphite) + 2 H₂ (g) C₂H₂ (g) 2. Calculate the AH for the reaction: Given CS (l) + 2 O (9) CO (9) * 2.SO, (B) AHCO₂ (g)-393.5 kJ/mol AHSO₂-296.8 kJ/mol AHCS₂(1) = 87.9kJ/mol
- The heat released when one mole of water is formed from the elements is 1,198 kJ. An experiment was conducted that permitted water to form in this manner, and the heat was contained in 2.0 liters of water. The water temperature before the reaction was 34.5°C, and after the reaction it had risen to 52.0°C. How many moles of water were formed? (The specific heat of water is 4.184 J/g·°C.)Answer: 0.12 mole (Can you explain how?)SIMPLE ALGORITHM: Solve the following problems. Write your answer on the space provided. Show your complete solutions. For your final answer, report correct significant figures and rounding off (Follow the conventional) 4. The value of ΔH0 for the reaction is -482 kJ. What is the heat released to the surroundings when 12.0 g of CO (g) reacts completely: 2CO(g) + O2(g) →2CO2(g) in kJ? 5. The value of ΔH0 for the reaction below is -186 kJ. Determine the heat released from the reaction of 25 g of Cl2: H2(g) + Cl2 → 2HCl(g) in kJ.SIMPLE ALGORITHM: Correct significant figures and rounding off (Conventional). 6. Given the following reactions: CaCO3(s) → CaO(s) + CO2(g) ΔH = 178.1 kJ C(s, graphite) + O2(g) → CO2(g) ΔH = -393.5 kJ Determine the enthalpy of the reaction of CaCO3(s) → CaO(s) + C(s, graphite) + O2(g).
- Simple Algorithm: Solve the following problems. Write your answer on the space provided. Show your complete solutions. For your final answer, report correct significant figures and rounding off (Follow the conventional). The value of ΔH0 for the reaction CH3OH(l) → CO(g) + 2H2(g) is +128.1 kJ. Determine the heat consumed when 5.10 g of H2(g) is formed.SIMPLE ALGORITHM. Correct significant figures and rounding off (Conventional). 9. In the reaction 2Al(s) + 3O2(g) → 2Al2O3(s), determine the ΔH0f of Al2O3(s) if the value of ΔH0 is -3351 kJ.Simple Algorithm: Solve the following problems. Write your answer on the space provided. Show your complete solutions. For your final answer, report correct significant figures and rounding off (Follow the conventional). 4. The value of for the reaction 2Ba(s) + O2(g)→ 2BaO(s) is -1107 kJ. Determine the amount of energy released when 5.75 g of BaO(s) is produced in kJ?
- Be sure to answer all parts. Deterioration of buildings, bridges, and other structures through the rusting of iron costs millions of dollars every day. Although the actual process also requires water, a simplified equation (with rust shown as Fe2O3) is: 4 Fe(s) + 3 O2(g) →2 Fe2O3(s) ΔHrxn = −1.65 × 103 kJ (a) What is the ΔHrxn when 0.250 kg of iron rusts? (b) How much rust forms when 4.20 ×103 kJ of heat is released?Simple Algorithm: Solve the following problems. Write your answer on the space provided. Show your complete solutions. For your final answer, report correct significant figures and rounding off (Follow the conventional). 3. The value of ΔH0 for the reaction: 2Ba(s) + O2(g)→ 2BaO(s) is -1107 kJ. What is the amount of energy released when 5.75 g of Ba(s) reacts completely with oxygen to form BaO(s) in kJ?Hi, I have a doubt. I'm doing my lab report: Thermochemistry and Specific Heat Capacity. I got stuck in the heat capacity. to solve this I have to use this formula qwater = mCp∆T, but I am not that specific heat capacityof water, I have to use 1calorie / gram ° C, or, 4.186 joules/gram ° C.Could you explain to me when I have to use each one? Here is my report, I don't need you to help me solve it, just explain my doubt please. Part 1: Determination of the Heat Capacity of a Calorimeter Water A Mass = 50.0 g Initial Temperature = 24.1°C Final Temperature = 28.7°C Specific heat capacity = 1 Cal /g °C Temperature change = 4.6 °C Heat of Water A (q) = 230 cal Water B Mass = 50.0 g Initial Temperature: 36.7 °C Final Temperature = 28.7 °C Specific heat capacity = 1 cal /g °C Temperature change = -8.0 °C Heat of Water B (q) = Calorimeter Heat of the Calorimeter = Initial Temperature = 24.1°C Final Temperature = 28.7 °C Temperature change = 4.6 °C Heat capacity (Kc) =…