Exp. 4 - Heat of Reaction

Consider the reaction: 2H₂O(1) 2H₂(g) + O₂(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.81 moles of H₂O(1) react at standard conditions. AS° surroundings = J/K

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J 3) If 4.00 g of iron metal are reacted in a calorimeter with a heat capacity of 400. C' what would be the final temperature of the calorimeter if its initial temperature were 23.0°C?

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Consider a hypothetical chemical reaction:     (In this equation   ,    ,     and     stand for some unknown chemical formulas.)   Here is an energy diagram for the reaction:     100 200 300 400   0         Consider a hypothetical chemical reaction:     (In this equation   ,    ,     and     stand for some unknown chemical formulas.)   Here is an energy diagram for the reaction:     100 200 300 400   0

Convert 475 cal to joules STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 4184 4.75 x 10° 1990 114 475 1000 1.99 x 10 0.001 4.184 kcal J kJ cal

- Question Completion Status. A Moving to another question will save this response. Question 1 Given the equation: CGH1206 + 602 - 6C02 + 6H20 AH =2864.6kJ Is the reaction exothermic or endothermic? How many kJ would be produced from the combustion of 60.77oz of C6H 120 6 (1 oz = 28.35 grams) round answer to the nearest whole number Moving to another question will save this response.

3-5: Heat of Combustion: Chicken Fat The heat of combustion (AHcomb) is the heat of reaction for the complete burning (reacting with O2) of one mole of a substance to form CO, and H,O. Calorimetry experiments that measure the heat of combustion can be performed at constant volume using a device called a bomb calorimeter. In a bomb calorimeter a sample is burned in a constant-volume chamber in the presence of oxygen at high pressure. The heat that is released warms the water surrounding the chamber. By measuring the temperature increase of the water, it is possible to calculate the quantity of heat released during the combustion reaction. In this assignment you will calculate the heat of combustion of chicken fat. The calorimeter has already been calibrated by combusting benzoic acid. 1. Start Virtual ChemLab, select Thermodynamics, and then select Heat of Combustion: Chicken Fat from the list of assignments. The lab will open in the Calorimetry laboratory with the bomb calorimeter out…

Please answer correct significant fig

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ΔH for the reaction IF5 (g) → IF3 (g) + F2 (g) is __________ kJ, given the data below. IF (g) + F2 (g) → IF3 (g) ΔH = -390 kJ               IF (g) + 2F2 (g) → IF5 (g) ΔH = -745 kJ Group of answer choices -35 +355 -1135 +1135 +35

At a certain temperature, the following reactions have the constant shown:   N2 (g)  + 2O2(g) ---> N2O4 (g)                                     Kc = 7.42 x 10-18                                              1/2N2 (g)   + O2 (g)  ----> NO2 (g)                                  Kc = 1.04 x 10-9   Calculate the Kc for each of the following: (Show your calculation on a piece of paper)   (a) 2NO2(g)      --->      N2(g)  +2O2   (b)  N2 (g)  + 2O2(g) ----> N2O4 (g)     (c)  2NO2(g) ---->   N2O4 (g)

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Hi! Can someone answer Learning task 4? Kindly include an explanation if applicable. Thanks!

Use the information below to answer questions 1- 3. PCI,(g) 2 PCI;(g) + Cl2(8) PCI,(g) decomposes into PCI,(g) and Cl,(8) according to the equation above. A pure sample of PCI,(g) is placed in a rigid, evacuated 1.00 L container. The initial pressure of the PCI5(g) is 1.00 atm. The temperature is held constant until the PCI,(g) reaches equilibrium with its decomposition products. The figures below show the initial and equilibrium conditions of the system. PCI5 Potal = 1.00 atm PCI5, PCI3, and CI, Prstal = 1.40 atm Figure 1: Initial Figure 2: Equilibrium As the reaction progresses toward equilibrium, the rate of the forward reaction (A) increases until it becomes the same as the reverse reaction rate at equilibrium (B) stays constant before and after equilibrium is reached (C) decreases to become a constant nonzero rate at equilibrium (D) decreases to become zero at equilibrium If the decomposition reaction were to go to completion, the total pressure in the container would be (A) 1.4…

Peisalla lamacron Nar. ,202 Date Name Section galauvinstenos Pre-Laboratory Assignment 1. Read an authoritative source for a discussion of preparing and interpreting a graph, especially the extrapolation of a curve. 2. A student determined the calorimeter constant of the calorimeter, using the procedure described in this module. The student added 50.00 mL of cold water to 50.00 mL of heated, distilled water in a Styrofoam cup. The initial temperature of the cold water was 21.00 °C and of the hot water, 29.15 °C. The maximum temperature of the mixture was found to be 24.81 °C. Assume the density of water is 1.00 g mL¯1 and the specific heat is 4.184 J g¯K gniwollot bns of toh bine botollon ot ssb om (1) Determine the AT for the hot water and the cold water. mit At cold water = 24.8I- 21,00 = 3.81°COn आनी AT hot = 24.81- 29.15 = - 4.34°C 60.ES 2.0 0LES 8. 0.1 0.0 If 0.8 28.5S Calculate N 0.4 08.TT gabxim 02 4.34°C hot water 81 answer cold water 381°C dogesn boximnu sdt to anuiSTeqmad mom…

Heat of Neutralization Initial temp of HCI solution Initial temp of NaOH solution Average initial temperature Final temp of neutralized mixture Change in temperature QH₂0 for the reaction (get mass using 50.0 mL solution and d= 1.02 g/mL) AHSolution (eqn 4) AH per mole istem brs 1915w to studseqmet munditiup3 25.9°C 24.9 °C 25.4 °C (E 360 m °C to on aitoaga 10.6 °C 2289.708 1 -2259.708 1 kJ/mol