Q: See image below. The answer I got is -626.58 kJ...is that correct?
A: Yes the answer which you got as per the given values is correct. The ΔH of the given reaction can be…
Q: Do exothermic or endothermic reactions have a greater tendency to be spontaneous, and why? IUse the…
A: A spontaneous reaction take place without any external input to the system. It can also be defined…
Q: For which reactions does entropy favor the products? (see attachment)
A: In Thermodynamics, entropy is a thermodynamic state function that is defined as the measure of the…
Q: If we define the system as the reactants and products, what is the sign of work in this process,…
A: According to the first law of thermodynamics, the internal energy of a system can be changed by…
Q: How much energy is transferred by 1 mol of 02(g) reacting in the equation below? C6) + ½ O2e) → CO),…
A: In this,half mole of oxygen react to release 110.5kj/mol of energy then when half mole of oxygen…
Q: AH° for the following chemical reactions are: so, (8) + H;O(1) → H;SO, (1) Bao (s) + so, (8) → Baso,…
A:
Q: using the information given below, calculate the Δ So at 25oC for the given reaction.…
A: Entropy change of a reaction can be calculated by sum of standard entropy of product - sum of…
Q: Enter your answer in the provided box. Consider the reaction H2g) + Ch@) → 2HCI(2) AH =-184.6 kJ/…
A:
Q: For the reaction below, determine the difference in relevant particles that allow for determination…
A:
Q: Predict the sign of ΔG for the following reaction conditions without using specific numbers:…
A: When the change occurs in the system, surroundings, and universe then automatically the value of…
Q: ₂0 and 0.444 J/g.°C for Fe. eat capacity of the calorimeter = 3/°C
A: The calorimetry rule says, Heat lost by iron = Heat gained by calorimeter + water Heat lost=mc∆T…
Q: For the chemical reaction below, determine the sign of the AS. Reaction Sign of AS (+ or -)…
A:
Q: Be sure to answer all parts. Deterioration of buildings, bridges, and other structures through the…
A: The balance chemical equation for rusting of iron is as follow 4Fe(s)…
Q: The enthalpy changes, AH, for three reactions are given. H, (g) + 0,®) – H,0) AH = -286 kJ/mol Са2+…
A: The 3 reactions given are, 1) 2) 3)
Q: Given the reactions, X(s)+12O2(g)⟶XO(s) Δ?=−676.5 kJ XCO3(s)⟶XO(s)+CO2(g)Δ?=+324.9 kJ what is Δ?…
A: Assuming the question is to find ΔH from the given reactions with there ΔH values as it is written…
Q: Use Equations a and b to determine ΔH for the following reaction.2CO(g) + 2NO(g) → 2C O 2 (g) + N 2…
A: The main equation or primary equation can be obtained by inverting equation (b) and then adding it…
Q: A 200 ml sample of 0.600 M aqueous hydrochloric acid is added to 300 mL of 0.400 M aqueous ammonia…
A:
Q: 7. Determine AH° for the following reaction: 2S(s) + 302(g) ---> 2SO3(g) AH°=? Given: SO2{g) --->…
A: 7) Given, a) SO2(g) ➝ S(s) + O2(g) ∆H° = +296.8 kJ b) 2SO2(g) + O2(g) ➝ 2SO3(g) ∆H° = -197.8 kJ…
Q: Consider the following balanced thermochemical equation for the decomposition of the mineral…
A: Thermochemical equation :- A chemical equation in which heat changes involved during the reaction…
Q: A hot (70°C) lump of metal has a mass of 250 g and a specific heat of 0.25 cal/g°C. John drops the…
A: heat lost by metal = heat gained by water + heatgained by calorimeter . m c T = m cT + m c T . 250…
Q: 0 70 Using tabulated thermodynamic data, calculate AG° for these reactions. (a) Mg,N,(s) + 6 H,0(()…
A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…
Q: Coal can be converted to methane, a chief component of natural gas, according to the following…
A:
Q: Cu(s) + 0.5 0; (g) --> CuO (s) DH - -275 kJ CuO(s) + Cu (s) --> Cu,O (s) DH = +64 kJ Calculate DH…
A:
Q: Calculate "q" (in kJ) for the following reaction if 11.35 grams of SO2(g) reacted with excess…
A: We have reaction of 11.35 g of SO2 with excess oxygen we have to calculate the q for this.
Q: A particular reaction has a ΔHo value of -169 kJ and ΔGo of -156 kJ at 524 K. Calculate ΔSo at 524 K…
A: The relation between ΔHo, ΔGo and ΔSo is shown below. ∆G∘=∆H∘-T∆S∘
Q: Calculate AHrn for Ca(s) + % Oz(g) + Co2 (g) → CaCO:(s) given the following set of reactions: Ca(s)…
A: Since you have asked multiple question, we will solve the first question for you. If you want any…
Q: Calculate “q” (in kJ) for the following reaction if 11.53 grams of O2(g) reacted with excess sulfur…
A:
Q: Consider the combustion of liquid methanol, ??3?? (?) CH3OH (l) + 3/2 O2 (g) → CO2 (g) + 2 H2O (l)…
A: Given reaction is : CH3OH (l) + 3/2 O2 (g) → CO2 (g) + 2 H2O (l) Enthalpy change of the reaction in…
Q: The value of AH for the reaction below is -482 kJ. Calculate the heat (kJ) released when 52.0 g of…
A: We can calculate the heat released by using stoichiometric calculation. We see from balanced…
Q: Use the following data to determine the AH° for the conversion c C(s,diamond) +O,(g) CO,(g) AH°=…
A: We will add all three equation to get final equation.
Q: If AGº is 137.1 kJ, ASº is -0.9 kJ/K and the T is 74.4 degrees celcius, find AH° is {enthalpy} kJ of…
A: Given information, ∆G0 = 137.1 kJ∆S0 = -0.9kJ/KT = 74.40C = 347.55 K
Q: At one time, a common means of forming small quantities ofoxygen gas in the laboratory was to heat…
A:
Q: 3. Calculate the AH for the reaction NO(g) + O(g) NO2(g) given the following information: NO(g) +…
A:
Q: Calculate AH for each of the following reactions (use the data in Appendix II): (a) 2 CH10 (g) + 13…
A:
Q: Calculate AH for the reaction, C,H,(g) + H,(g) → C,H,(g) Given: (a) 2 C,H,(g) + 5 0,(g) →4 CO,(g) +2…
A:
Q: For the reaction Co(g) + 3H2(g)CH4(g) + H20(g) AH° = -206.1 kJ and AS° = -214.7 J/K The maximum…
A:
Q: Be sure to answer all parts. Deterioration of buildings, bridges, and other structures through the…
A: Given Data: *Mass of iron rust formed is 0.250 Kg or 250 g in (a) part. *Enthalpy of reaction is…
Q: The value of ΔHo for the following reaction is -72 kJ. How many kJ of heat will be evolved when 4.0…
A:
Q: 2. Calculate AH for the reaction: CH4 (g) + 4 Cl2 (g) CCI4 (g) +4 HCI (g) Use the following…
A: We have to calculate ∆Hrxn for the reaction CH4(g) + 4Cl2(g) → CCl4(g) + 4HCl(g).
Q: For the reaction 4HCI(g) + O2(g) 2H20(g) + 2C12(g) AH° = -114.4 kJ and AS° = -128.9 J/K The maximum…
A:
Q: Silver bromide is used to coat ordinary black-and-white photographic film, while high-speed film…
A:
Q: If you have a reaction that occurs in aqueous solution, and raises the temperature of 15.9 g of…
A: As the reaction is exothermic , it liberates heat which rises the temperature of water so sign of…
Q: How much work in L*atm is done by 1.44 moles of a gas that has an initial volume of 22.5 liters and…
A: Initial Volume of gas = 22.5 L Calculation of final volume of gas: where P is the final pressure, V…
Q: How much heat is released at constant pressure if 12.3 mL of 0.161 M silver nitrate is mixed with…
A: Given, AgNO3(aq) + KCl(aq) ➝ AgCl(s) + KNO3(aq) ∆H° = -65.5 kJ Here (-) sign indicate the release…
Q: Calculate the ΔGo for a reaction, given the ΔHo for the reaction = -5052.8 kJ and the ΔSo for the…
A: Recall the following expression to calculate∆G° as follows ∆G°=∆H°-T∆S°Given…
Q: 12. Copper() oxide can be oxidized to copper(II) oxide: Cu20(s) + % O2(g) →2CuO(s) AH ran = - 146.0…
A:
Q: Calculate H,O (g) + C (s) - CO (g) + H, (g) Using Eqn i H, (g) + 1/2 0, (g) → H,O (g) AH Eqn 2 2C0…
A: Heat of a reaction is given by the heat of formation of products minus that of the reactants.
Step by step
Solved in 2 steps with 1 images
- Define the standard enthalpy of formation. What are standard states for elements and for compounds? Using Hess's law, illustrate why the formula Hreaction=npHf(products)nfHf(reactants) works to calculate H for a reaction.Given the following data 2O3(g) 3O2(g)H = 427 kJ O2(g) 2O(g)H = 495 kJ NO(g) + O3(g) NO2(g) + O2(g)H = 199 kJ Calculate H for the reaction NO(g) + O(g) NO2(g)How is the sign of q, heat, defined? How does it relate to the total energy of the system?
- For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate G . (Assume that both enthalpy and entropy are independent of temperature.)The overall reaction that occurs when sugar is metabolized is C12H22O11(s)+12O2(g)12CO2(g)+11H2O(l) For this reaction, H° is -5650 kJ and G° is -5790 kJ at 25°C. (a) If 25% of the free energy change is actually converted to useful work, how many kilojoules of work are obtained when one gram of sugar is metabolized at body temperature, 37°C? (b) How many grams of sugar would a 120-lb woman have to eat to get the energy to climb the Jungfrau in the Alps, which is 4158 m high? ( w=9.79103mh, where w= work in kilojoules, m is body mass in kilograms, and h is height in meters.)Shown below is a diagram depicting the enthalpy change of a chemical reaction run at constant pressure. a Is the reaction exothermic or endothermic? b What is the sign of H? c What is the sign of q? d If the reaction does no work, what is the sign of E for this process?
- Athletic trainers use instant ice packs that can be cooled quickly on demand. Squeezing the pact breaks an inner container, allowing two components to mix and react. This reaction makes the pack become cold. Describe the heat flow for this spontaneous process.9.83 A student performing a calorimetry experiment combined 100.0 mL of 0.50 M HCl and 100.0 mL of 0.50 M NaOH in a coffee cup calorimeter. Both solutions were initially at 20.0°C, but when the two were mixed, the temperature rose to 23.2°C. (a) Suppose the experiment is repeated in the same calorimeter but this time using 200 mL of 0.50 M HCl and 200.0 mL of 0.50 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why? (b) Suppose that the experiment is repeated once again in the same calorimeter, this time using 100 mL of 1.00 M HCl and 100.0 mL of 1.00 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why?Nickel metal reacts with carbon monoxide to form tetra-carbonyl nickel, Ni(CO)4: Ni(s)+4CO(g)Ni(CO)4(g) This reaction is exploited in the Mond process in order to separate pure nickel from other metals. The reaction above separates nickel from impurities by dissolving it into the gas phase. Conditions are then changed so that the reaction runs in the opposite direction to recover the purified metal. (a) Predict the sign of S for the reaction as written above. (b) Use tabulated thermodynamic data to calculate H, S , and G for the reaction. (c) Find the range of temperatures at which this reaction is spontaneous in the forward direction.
- Coal is used as a fuel in some electric-generating plants. Coal is a complex material, but for simplicity we may consider it to be a form of carbon. The energy that can be derived from a fuel is sometimes compared with the enthalpy of the combustion reaction: C(s)+O2(g)CO2(g) Calculate the standard enthalpy change for this reaction at 25C. Actually, only a fraction of the heat from this reaction is available to produce electric energy. In electric generating plants, this reaction is used to generate heat for a steam engine, which turns the generator. Basically the steam engine is a type of heat engine in which steam enters the engine at high temperature (Th), work is done, and the steam then exits at a lower temperature (Tl). The maximum fraction, f, of heat available to produce useful energy depends on the difference between these temperatures (expressed in kelvins), f = (Th Tl)/Th. What is the maximum heat energy available for useful work from the combustion of 1.00 mol of C(s) to CO2(g)? (Assume the value of H calculated at 25C for the heat obtained in the generator.) It is possible to consider more efficient ways to obtain useful energy from a fuel. For example, methane can be burned in a fuel cell to generate electricity directly. The maximum useful energy obtained in these cases is the maximum work, which equals the free-energy change. Calculate the standard free-energy change for the combustion of 1.00 mol of C(s) to CO2(g). Compare this value with the maximum obtained with the heat engine described here.Some water is placed in a coffee-cup calorimeter. When 1.0 g of an ionic solid is added, the temperature of the solution increases from 21.5C to 24.2C as the solid dissolves. For the dissolving process, what are the signs for Ssys, Ssurr, and Suniv?For the reaction C2H2(g)+4F2(g)2CF4(g)+H2(g) S is equal to 358 J/K. Use this value and data from Appendix 4 to calculate the value of S for CF4(g).