Determine the higher heating value of n-butane, according to its gas phase with and without condensation of the water vapor formed, and at p=cte or V=cte.
Q: In a 6.00 L pressure cooker, water is brought to a boil. If the final temperature is 115 °C at 3.85…
A: Volume=6.00L Temperature= 115°C=(115+273)K=388K Pressure=3.85 bar R=0.08314L-bar/mol-K
Q: An isothermal compression is done on 3.27 mol of an ideal monoatomic gas at 88.6°C in a diathermic…
A: Formula used:- W= 2.303nRT log V2/V1 Thus for isothermal process Q = -W
Q: H.W) 1013.25 J of heat energy is supplied to 1mol of NH3 (2) which is initially volume is 4L at…
A:
Q: 1.30. Determine the expressions for the following, assuming that the ideal gas law holds. an (27),…
A: Ideal Gas equation is given by:PV = nRTwhere, P is pressureV is Volumen is number of milesR is…
Q: Irreversible Isothermal Compression, Van der Waals Gas Suppose 2.0 mol of CO2(g) undergoes an…
A:
Q: One mole of gas expands isothermically to double its volume. If the gas temperature is 320 K, what…
A: Temperature (T) = 320 K Number of moles = 1mol Volume(V2) = 2 volume (V1)
Q: Calculate the values of internal energy change and entalphy change for heating 55.40 g of xenon from…
A:
Q: Calculate the change in the internal energy when when 2.5 mol of CO₂ (assumed 2 to det like a van…
A: Calculate the change in the internal energy when when 2.5 mol of CO2 (assumed 2 to det like a van…
Q: A vessel containing 39.6 cm3 of helium gas at 25 C was inverted and placed in cold liquid ethanol.…
A: According to Charles's law, the volume of the gas increases when the temperature of the gas…
Q: Calculate the change in molar enthalpy of carbon dioxide assoicaited with raising the temperature of…
A: The question can be solved by using integration. The detailed solution is shown below.
Q: Irreversible Isothermal Compression, Van der Waals Gas Suppose 2.0 mol of CO2(g) undergoes an…
A: For n moles Van der Waals's gas, (P + n2a/v2) (v - nb) = nRT…
Q: Determine the temperature of the combustion product of 1 L of bioethanol if the heat from the…
A: The objective of this question is to show the determine the temperature of the combustion products.…
Q: how much heat Q needs to be supplied to the gas?
A: In this question wh have to calculate the heat Q needs to be supplied to the gas with teh help of…
Q: The molar heats of formation of liquid and gas phase water are given by: kJ H₂ (9) + 02 (9) → H₂O(l)…
A: The enthalpy change is a state function and the Hess law states that the change of enthalpy in a…
Q: At 1 atm, how much energy is required to heat 95.0 g H2O(s)] at −14.0 ∘C to H2O(g) at 115.0 ∘C? Use…
A: Mass of water = 95.0g Specific heat of ice = 2.087J/g°C ∆Hfusion = 333.6J/g Specific heat capacity…
Q: QUESTION 16 Which of the following is an assumption of Kirchoff's law for a defined temperature…
A: Kirchoff's Law states that the enthalpy of the reaction varies with the temperature changes.
Q: What is the state of a system that has a system pressure of 500 mmHg and a dew pressure of 622 mmHg…
A: We can define the dew pressure as the pressure of the system where appearance of liquid occurs from…
Q: Equimolar ethylene gas and steam at 593.15 K at 1 atm are fed to a reaction process to produce…
A: We need to find the heat transfer associated with the reaction of ethylene gas to produce ethanol,…
Q: One mole of gas expands isothermically to double its volume. If the gas temperature is 340 K, what…
A:
Q: The heat capacity of a diatomic gas fits the expression Cp = a + BT + yT² + ST³ . The values of the…
A:
Q: * Quesbon Moving to another question will save this response. Quèstion 3 For a real gas, when…
A: Explained as follows
Q: A particular gas cylinder will explode if the pressure exceeds 14×103KPa.The cylinder has a capacity…
A:
Q: Solve please, I'm confused with part a, better to solve both.(AI answer not allowed). A 2.50 g…
A: a) During thermal equilibration, the system consisting of copper and air will reach thermal…
Q: Q7. A sample consisting of 1 mol of perfect gas atoms (for which Cy=R) is taken through the cycle…
A: The main aim of this question is to calculate the q. w, AU, and H for each step and for the overall…
Q: How much heat is required when 2,000 kg of C3H6 is heated at atmospheric pressure from 50°C to 830…
A: Heat energy required or released can be calculated by using the formula: Q = n×Cp×ΔT -----(1) Where…
Q: (CLO3 A saturated mixture state is O less than 100% vapor O50% liquid and 50% vapor 10% vapor and…
A: Ans of the question a saturated mixture state is-
Q: Complete the equations
A: Carbenes Carbenes are the electron deficient reaction intermediates in which both lone pair of…
Q: steam A vessel of volume 8.7m³ contains air and dry saturated steam (Pste 34.8m³/kg) at a total…
A:
Q: A 0.513 mol sample of NO2(g) initially at 298 K and 1.00 atm is held at constant volume while enough…
A: From 1st law of thermodynamics, we come to know that energy cannot be created or destroyed. It can…
Q: A body of experimental evidence suggest that I addition, an ideal gas also obeys the equation of…
A: First of all calculate the relation between P, V and T from the ideal gas equation. Then a relation…
Q: An isothermal compression is done on 1.42 mol of an ideal monoatomic gas at 15.8°C in a diathermic…
A: The question is based on the concept of chemical thermodynamics. We have to calculate heat involved…
Q: Part A: Methane at low temperatures Methane (CH4) is a tetrahedral molecule. Determine its specific…
A: We need to calculate the molar heat capacity at constant volume for a polyatomic gas, methane (CH4).…
Q: A cyclinder fitted with a piston holds 8.07g CH4 in 7.05L at -8C. While heating the gas at 1.55atm,…
A: Given, Volume of sample is 7.05 L Initial temperature = -8 oC = 273 - 8 = 265 K Pressure = 1.55 atm…
Q: Pbis + SOao, (0.30M) + 24gCl → PbSO4 + 24g + 2Cliae) (0.20M) PbSO4 + 24gs + 2C1ia) 4(ag)
A: Concentration of pure solids, pure liquids are omitted from equilibrium constant expression because…
Q: 5. At its normal boiling point (337.3 K), methanol (CH3OH) has AvapH = 25.79 kJ/mol, and the…
A: As per Clausius-Clapeyron equation, dPdT=∆HT∆V
Q: In a 6.00 L pressure cooker, water is brought to a boil. If the final temperature is 115 °C at 3.15…
A: P V = n R T Where P = 3.15 bar V = 6 L n = moles = ? R = 0.08314 L bar /mol k T = 115° C = 115…
Q: 5. Hydrogen gas burning in excess from oxygen gas in H2g + 1002g +→ H2O + excess O2g The heat of…
A: To solve these problems, we need the following equations: 1. The Kirchhoff's equations:…
Q: Acetylene (C2H2), which is used for industrial welding, is transported in pressurized cylinders. Its…
A: The vapour pressure v/s temperature data given is,
Q: At 1 atm, how much energy is required to heat 75.0 g H2O(s) at −14.0 ∘C to H2O(g) at 123.0 ∘C? Use…
A: We will write all conversion steps and calculate heat required for each step and add them up.
Q: If 293 J of heat is required to raise the temperature of 2 mol of an ideal gas at constant pressure…
A:
Q: nder hasa ptn that movesnor necsarke constat presure on he mref. The nders ergednage ed wter See…
A: The given experiment is based on the application of the first law of thermodynamics.
Q: Given these relation, prove this without usin Maxwell relatios (), = -(), P
A: This is a simple problem of just using thermodynamic relations to equate two differential equations…
Q: In a certain combustion of methane in a combustion chamber using excess air, an issue occurred,…
A: The heat of combustion is viewed as a calorific value, which can be described as the complete…
Q: From fundamental property relations, proof the following equation is valid. as aP T.
A: We have to prove the given expression using the fundamental equation.
Q: Titanium has an allotropic transformation form HCP to BCC at 915 °C. If the HCP c/a ratio is 1.58…
A: The ration of c to a is 1.58 The number of atoms per unit cell in HCP = 6 Atomic weight of Titanium…
Q: (a) Compute R for the following three gasses: (i) Ethane (C2H6) (ii) Helium (He) (iii) Oxygen (O2)…
A: The product of pressure and volume is the definition of the gas constant. It is given as energy per…
Q: In a 6.00 L pressure cooker, water is brought to a boil. If the final temperature is 115 °C at 4.25…
A: Given Volume ( V ) = 6 L Temperature ( T ) = 115 ℃ = ( 115 + 273…
Determine the higher heating value of n-butane, according to its gas phase with and without condensation of the water vapor formed, and at p=cte or V=cte.
![](/static/compass_v2/shared-icons/check-mark.png)
Step by step
Solved in 3 steps with 20 images
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
- What fraction of the water vaporization enthalpy is consumed in the expansion of water vapor?True or False (2) In thermochemical equations, it only shows the direction of the reaction involved. (5) The decomposition of ozone by nitric oxides homogeneous catalysis can be represented in the reaction: O(g) + O3(g) + NO(g) → 2O2 (g). (666) The negative energy indicates its flow. (121212) The CH3COOH could have greater vapor pressure lowering than NaOH. (131313) The temperature of the substance can influence its concentration. (252525) An insect can crawl in the surface of the water because of the strong intermolecular forces of attraction between the liquid and the insect’s legs. (313131) The rate of reaction can be defined as the change in the positive change in the concentration of product and reactants per change in time. (323232) The colligative properties depend on the concentration based on the solvent (34343434)Q2:-Correct the following Statements: 1)The thermal coefficient of expansion is only a function of temperature. 2)the latent of vaporization is increasing with heating. 3)The melting point of waxes is when crystals start appearing . 4)The high thermal properties does not affect molecular weights of H.C. 5)Final boiling point( FBP ) is constant for all C.O products.
- Calculate the amount of energy in the form of heat that is produced when a volume of 4.37 L of SO2(g) is converted to 4.37 L of SO3(g) according to this process at constant pressure and temperature of 1.00 bar and 25.0 ° C. Assume ideal gas behavior.Irreversible Isothermal Compression, Van der Waals Gas Suppose 2.0 mol of CO2(g) undergoes an irreversible isothermal compression at 400 K from 20.0 L to 15.0 L using an external pressure of 30.0 bar. Assume van der Waals gas behavior. For CO2: a = 3.610 atm dm6 mol-2 b = 0.0429 dm3 mol-1 ΔU= ∫ V2 V1 (an^2/V2)dV If ΔU = -24 J, what is the numeric value of q (in joules)?Irreversible Isothermal Compression, Van der Waals Gas Suppose 2.0 mol of CO2(g) undergoes an irreversible isothermal compression at 400 K from 20.0 L to 15.0 L using an external pressure of 30.0 bar. Assume van der Waals gas behavior. For CO2: a = 3.610 atm dm6 mol-2 b = 0.0429 dm3 mol-1 ΔU= ∫ V2 V1 (an^2/V2)dV
- An isothermal compression is done on 1.42 mol of an ideal monoatomic gas at 15.8°C in a diathermic balloon very slowly so that its final volume is half its initial volume. What is the heat of this process? Enter your answer in units of Joules to zero decimal places.In this assignment, we will consider 1 mole of N2(g) which is in a closed container. In state 1, the temperature is 25°C and the pressure in the container is 10 bar.We assume that N2 behaves like an ideal gas and that Cp,m(g) = 29.125 J mol-1K-1, and is independent of temperature. 1) How large will a) the volume work, b) the heat and c) the change in enthalpy of N2 be if, starting from state 1, the volume of the container was changed in a reversible and isothermal manner so that the pressure in the container drops to 1 bar? 2) How big will a) the volume work, b) the heat and c) the change in enthalpy of N2 be if, again starting from state 1, the volume of the container was changed in a reversible and adiabatic way so that the pressure in the container drops to 1 bar? 3) a) Explain what reversible means in tasks 1) and 2) b) state what the change in the entropy of the universe is in tasks 1) and 2). 4) How large will a) the volume work, b) the heat and c) the change in enthalpy of N2…the ionic compound L2O3(s) is the ionic compound formed from oxygen and a metal with the form L(s) at 1.00 bar and 298 K. (a) Draw the Lewis structure for L2O3. Assume that all the valence electrons from L are required. (b) Use the following information to determine the enthalpy of formation for L2O3(s). Express your answer in kJZ(mol L2O3(s)). Lattice energy for L2O3(s) = -14836 kJ mol1 AHsub for L(s) = 358 kJ mol 1 First ionization energy for L(g) = 577 kJ mol 1 Second ionization energy for L(g) = 1794 kJ mol 1 Third ionization energy for L(g) = 3820 kJ mol 1 Bond dissociation energy for O2(g) = 498 kJ mol 1 %3D First electron affinity for O = -141 kJ mol 1 Second electron affinity for O = 744 kJ mol 1
- 2.00-mol of a monatomic ideal gas goes from State A to State D via the path A→B→C→D: State A PA=13.5atm, VA=11.50L State B PB=13.5atm, VB=7.00L State C PC=25.0atm, VC=7.00L State D PD=25.0atm, VD=25.00L Assume that the external pressure is constant during each step and equals the final pressure of the gas for that step. Calculate q for this process. Calculate w for this process. Calculate ΔE for this process Calculate ΔH for this process.2.00-mol of a monatomic ideal gas goes from State A to State D via the path A- > B-> C-> D: State A PA = 11.0atm, VA = 13.50L State B PB = 11.0atm, VB = 6.00L State C PC = 25.0atm, VC = 6.00L State D PD = 25.0atm, VD = 20.50L Assume that the external pressure is constant during each step and equals the final pressure of the gas for that step. Calculate q for this process.Determine the number of degrees of freedom (trans + rot) for each of the following gases; Ne, CO2, H2O. Then calculate the average total kinetic energy (per mole) at 25 celsius for each gas. (R=8.314J K-1 mol-1)
![Principles of Modern Chemistry](https://www.bartleby.com/isbn_cover_images/9781305079113/9781305079113_smallCoverImage.gif)
![Physical Chemistry](https://www.bartleby.com/isbn_cover_images/9781133958437/9781133958437_smallCoverImage.gif)
![Principles of Modern Chemistry](https://www.bartleby.com/isbn_cover_images/9781305079113/9781305079113_smallCoverImage.gif)
![Physical Chemistry](https://www.bartleby.com/isbn_cover_images/9781133958437/9781133958437_smallCoverImage.gif)