SIMPLE ALGORITHM. Correct significant figures and rounding off (Conventional). 7. Given the following reactions N2(g) + O2(g) → 2NO(g) ΔH = +180.7 kJ 2N2O(g) → O2(g) + 2N2(g) ΔH = -163.2 kJ Determine the enthalpy of reaction: 2N2O(g) → 2NO(g) + N2(g).
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SIMPLE ALGORITHM. Correct significant figures and rounding off (Conventional).
7. Given the following reactions
N2(g) + O2(g) → 2NO(g) ΔH = +180.7 kJ
2N2O(g) → O2(g) + 2N2(g) ΔH = -163.2 kJ
Determine the enthalpy of reaction: 2N2O(g) → 2NO(g) + N2(g).
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- The enthalpy of combustion of isooctane (C8H18(l)) is -5461 kJ/mol. From data found in appendix G, calculate the enthalpy of formation of C8H18(l): C8H18(l) + 12.5 O2(g) → 8 CO2(g) + 9 H2O(l) ∆Hrxn = -5461 kJ ∆Hf = ___ kJ/mol Correct answer is not 259.2Please assist me with my practice question. The combustion of butane is shown by the following equation: 2C4H10 (l) + 13O2 (g) → 8CO2 (g) + 10H2O(g) Use the following data and the summing method to find the heat of reaction for the above equation. Note: Show all calculations, follow the rules of significant figures, and box your final answer. C(s) + O2 (g) → CO2 (g) + 393 kJ H2 (g) + ½O2 (g) → H2O(g) + 242 kJ 4C(s) + 5H2 (g) → C4H10 (g) + 125 kJCalculate the weight (number of pounds) of each rank of coal that would have to be burned to produce 3.5 million BTU (or 3,500,000 BTU) of heat, using the data in the table. Because a range of heating values (or energy output) is given for each coal rank, include a range in your answers. Put your answers in the column on the right, in the table below. Sample problem: 1.00 × 10⁶ × 1.00 lb/5.50 × 10³ BTU × 1kg/2.20 lbs = 82.6 kg 1.00 × 10⁶ BTU × 1.00 lb/8.30 × 10³ BTU × 1kg/2.20 lbs= 54.76 kg
- what mass of iron do you have (in g) if 257.7 J of heat causes an increase of 3.37°C? the specific heat if iron is 0.449 J/gK =0.449J/g°C give answer in standard notation with no decimal placesMetal Specific Heat (J/goC) Calcium 0.647 Iron 0.449 Silver 0.235 Gold 0.129 In joules, how much heat is released when 47.0 g of Ag cools from 199. to 123.? Answer: -_______ J (enter a positive value)A 102.3-g sample of vodka is burned with excess oxygen in a bomb calorimeter with a heat capacity of 15.3 kJ·K–1. The temperature of the calorimeter rises from 21.15°C to 82.09°C. What is the ΔUrxn value for the combustion of this vodka sample in units of kJ/g? Enter your numerical answer only (no units) to the correct amount of significant figures.
- The specific heat of lead is 0.129 J/g-oC. How many joules of heat is required to raise the temperature of 284g of lead from 22.25oC to 29.94oC? (Final answer: ONE decimal place)an important flavor component of vanilla extract is vanillin C8H8O3 molar mass = 152.15 g/mol when vanillin burns in a bomb calorimeter with a heat capacity of 12.16 kJ/ celsius the temp increases from 24.56 celsius to 30.60 celsius. if the heat of combustion of vanillin is -3760 kJ/mol what mass of vanillin (in g) was combusted? answer to two decimal placesan important flavor component of vanilla extract is vanillin C8H8O3 molar mass = 152.15 g/mol when vanillin burns in a bomb calorimeter with a heat capacity of 8.60 kJ/°C the temp increases from 25.97°C to 31.18°C. if the heat of combustion of vanillin is -3760 kJ/mol what mass of vanillin (in g) was combusted? answer to two decimal places
- Which element in the periodic table has an specific heat of 0.099 with the lowest percentage errorA 50.15 g of iron with an initial temperature of 100.26°C was put in 105.73 g of ethanol (specific heat of ethanol = 2430 J/kg∙K) with an initial temperature of 20.11°C. The final temperature of the system (assuming there's no heat exchange between the container, thermometer, and the environment) is 26.45°C. If you are asked to compute for the experiment value of the specific heat of the iron, how much is the percent error of the experiment (accepted/standard value of the specific heat of iron is 448 J/kg∙K)? less than 1% between 1% to 5% between 5% to 10% more than 10%* Please I want answer of these questions (All Sub-parts) as urgent basis. Many Thanks. 430 grams of copper pellets are removed from 330°C oven and immediately dropped into 250 mL of water in an insulated cup. The temperature of water raises 39°C then remains at that temperature. Calculate the following: a) Mass of water in kilograms b) The heat energy removed from copper pellets in joules . (Sp.Heat of copper is 385 J/Kg°C) c) The initial temperature of water in degree celsius . (Sp.Heat of water = 4186 J/kg°C)