Octane (C8H18) is a component of gasoline and combusted according to the reaction below. Is the reaction exothermic or endothermic and what is the change in heat energy if 34.5 g of octane is combusted with excess oxygen? (Note: the molar mass of octane is 114.2 g/mol) 2C3H18 (1) + 2502 (g) → 16CO2 (g) + 18H20 (g) AH= -10860 kJ O exothermic, -3280 kJ O exothermic,-10860 kJ O exothermic, -1640 kJ O endothermic, -1640 kJ O endothermic, -3280 kJ

Octane (C8H18) is a component of gasoline and combusted according to the reaction below. Is the reaction exothermic or endothermic and what is the change in heat energy if 34.5 g of octane is combusted with excess oxygen? (Note: the molar mass of octane is 114.2 g/mol) 2C3H18 (1) + 2502 (g) → 16CO2 (g) + 18H20 (g) AH= -10860 kJ O exothermic, -3280 kJ O exothermic,-10860 kJ O exothermic, -1640 kJ O endothermic, -1640 kJ O endothermic, -3280 kJ

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

When sulfuric acid dissolves in water, a great deal of heat is given off. The enthalpy change for this process is called the enthalpy of solution. To measure it, 175.0 g of water was placed in a coffee-cup calorimeter and chilled to 10.0 °C. Then 49.0 g of pure sulfuric acid, also at 10.0 °C, was added, and the mixture was quickly stirred with a thermometer. The temperature rose rapidly to 14.9 °C. Assume that the specific heat capacity of the resulting sulfuric acid solution is 4.19 J/g °C. Calculate the quantity of thermal energy transferred, Q, for the formation of this solution, and calculate the molar enthalpy of solution in kilojoules per mole of H₂SO4.
Which equation is correct for the formation reaction of nitric acid, HNO3? A) N₂(g) + H₂(g) + 30₂(g) → 2HNO3(aq) ΔΗ = 174 kJ B) N₂(g) + H₂(g) + 30₂(g) → 2HNO3(0) AH = -174 kJ C) NH3(g) + N₂(g) + 30₂(g) → 3HNO3(aq) D) 1/2N₂(g) + 1/2H₂(g) + 3/20₂(g) → HNO3(/) 1 E) N₂(g) + H₂(g) + O₂(g) → HNO3(/) ΔΗ = 174 kJ ΔΗ = -174 kJ ΔΗ = -174 kJ
30 g of HCL is mixed with 200 g of water. The water temperature changes from 24.6 to 28.2 °C. What was the heat change (enthalpy change) of the water?
Calculate the heat of reaction (in J)
When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
They are all one question. In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction.A student heats 60.42 grams of chromium to 98.12 °C and then drops it into a cup containing 82.86 grams of water at 23.37 °C. She measures the final temperature to be 28.57 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.80 J/°C.Assuming that no heat is lost to the surroundings calculate the specific heat of chromium.Specific Heat (Cr) = ______J/g°C. In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction.Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is…
If 2.36 g of calcium dichloride dissolves in 84.00 g of water in a kalorimeter at a constant pressure, the temperature increases from 18.000C to 19.279C. Assuming that the kalorimeter absorbs no heat and the specific heat of the solution is the same as that of water (SpHt = 4.184 J/g C). What is the heat change of the solution of calcium chloride in units of kj/mol calcium dichloride? Please show step by step work.
In a coffee-cup calorimeter, 120.0 mL of 1.4 M NaOH and 120.0 mL of 1.4 M HCL are mixed. Both solutions were originally at 20.6°C. After the reaction, the final temperature is 30.0°C. Assuming that all the solutions have a density of 1.0 and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCL by NaOH . Assume that no heat is lost to the surroundings or to the calorimeter. ΔH = kJ/mol
If 0.064 mol of hydrochloric acid (HCl) is mixed with 0.064 mol of sodium hydroxide (NaOH) in a "coffee cup" calorimeter, the temperature of 4.9 g of the resulting solution increases from 25.0°C to 30.0°C.Given that the energy released is 1.2 × 101 cal when the specific heat of the resulting solution is 1.00 cal/g−°C, use a conversion factor to convert the energy released to joules (J).
8. Instant cold packs can be made from ammonium nitrate by mixing/reacting it with water (reaction shown below). When 1.25 g of NH4NO3 is dissolved in 25.0 g of water at 25.8 °C, the temperature of the water after the reaction is 21.9 °C. What is the enthalpy change (ΔH) for this reaction in units of kJ/mol of NH4NO3? The heat capacity of water is 4.18 ?/ ?℃ . NH4NO3(s) → NH4+(aq) + ??3 − (aq)
can you please solve part c and d
In the following reaction, how many grams of CH3OH are required to produce 1.578 x 10° kJ of heat? 2 CH3OH (1) +3 O2 (g) → 2 CO2 (g) + 4 H2O(g) AH = -1280. kJ/mol Please do not include units in your answer.