Practice Problem CONCEPTUALIZE The diagrams represent systems before and after two related chemical reactions. The heat of reaction for the first is -1755.0 kJ. Determine the heat of reaction for the second. heat of reaction = -1755.0 kJ before after heat of reaction = ? before after
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- What is the work when a gas expands from 0.666 L to 2.334 L against an external pressure of 2.07 atm? Note: answer is in Joules.The value of ΔH° for the reaction below is -126 kJ. The enthalpy change accompanying the reaction of 36 g of Na2O2 with water is __________ kJ. 2Na2O2 (s) + 2H2O (l) → 4NaOH (s) + O2 (g) The molar mass of Na2O2 is 77.98 g/mol. Include sign if answer is negative.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?)
- The ΔHreaction for the combustion of ethanol (CH3CH2OH) is -1,370.7 kJ/mol. If 100.0 g of ethanol (CH3CH2OH) reacts with 3.000 X 1024 molecules of oxygen gas, how kJ of heat will be released? Show work/to really explain approach please.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 kJHow can I calculat ethe number of KJ required for a reaction when give grams it begins with and Hrxn? example problem: Calculate the number of kJ required for the reaction shown below, if you begin with 63 grams of calcium carbonate (CaCO3), and the ΔHrxn = 178 kJ. CaCO3(s) → CaO(s) + CO2(g)
- Heat is added to a system, and the system dose 52 J of work. If the internal energy increase by 14 J, how much heat was added to the system? Show procedure and the final resultMethane reacts with oxygen at constant pressure CH4 (g) + 2O2 (g) → 2H2O (l) + CO2 (g) DH = -890 kJ / mol Is this an exothermic or endothermic reaction? (basically answer) Will change in inner energy, YOU be greater or smaller than DH? (basically answer) How much heat is transferred when 4.50 g of methane reacts?need it fast! For the balanced thermochemical equation below: 2 Mg(s) + O2(g) → 2MgO(g) ∆Hfo (MgO) = -601.8 kJ. Assuming 40.0 g of oxygen gas is consumed in the presence of an excess amount of magnesium, how much heat in kJ is evolved (sign is assumed to be negative for heat evolved; do not include the sign). Report to the nearest 0.1 kJ.
- Direction: Find the following ΔH for the reaction below. Topic: Hess's LawSimple 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?Hydrogen gas and oxygen gas release 482.6 kJ of heat when they combine to form steam. Is this reaction endothermic or exothermic? In which direction does heat transfer (between system and the surroundings) for this reaction? Is ΔH for this reaction positive or negative? topic: enthalphy of reaction