Part Cnd....pdfΔΗ = - - 123 kJ; ASn ==Express your answer as an integer.AGixn=SubmitPart D| ΑΣΦRequest AnswerAH-123 kJ; ASixn == 244 J/K; T = 615 KExpress your answer as an integer.244 J/K; T = 290 K15. ΑΣΦ 5 →P PearsonP IMG 5023 (1).pdfMacBook Air?on Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us |kJReview I Conspr 23 2032 tes....mwx

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ΔΗ, Π = − 123 kJ; ΔSx = – 244 J/K;T = 290 K == Express your answer as an integer. AGixn = Submit Part D 15. ΑΣΦ Request Answer ΔΗ – 123 kJ; ΔSix Express your answer as an integer. IVE ΑΣΦ 195 -- = ~ 244 J/K; Τ = 615 Κ IMG_5023 (1).pdf -- 3 → ? ? kJ P Pearson tion Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us | spr 23 2032 tes....mwx

ΔΗ, Π = − 123 kJ; ΔSx = – 244 J/K;T = 290 K == Express your answer as an integer. AGixn = Submit Part D 15. ΑΣΦ Request Answer ΔΗ – 123 kJ; ΔSix Express your answer as an integer. IVE ΑΣΦ 195 -- = ~ 244 J/K; Τ = 615 Κ IMG_5023 (1).pdf -- 3 → ? ? kJ P Pearson tion Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us | spr 23 2032 tes....mwx

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.88E: The following are values of heat capacity for nitrogen gas; Temp K Cv J/mol. K 300 20.8 400 20.9 500...

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The following are values of heat capacity for nitrogen gas; Temp K Cv J/mol. K 300 20.8 400 20.9 500 21.2 600 21.8 700 22.4 800 23.1 900 23.7 1000 24.3 1100 24.9 Using the general formula Cv = A BT C/T2, find values of A, B, and C that fit the given data.
The heat capacity (Cp) 0f an hal0genated 0rganic c0p0und, chl0r0f0rm is given by the f0ll0w equati0n. Equati0n (1) Cp (J/mol K) = 19.8 +0.22 T – 0.00026 T2 (a) 0btain a new equati0n that uses T in Fahrenheit (b) Calculate the Cp 0f chl0r0f0rm at 300 K using Equation (1) (c) Calculate the Cp 0f chl0r0f0rm at 80 F using the equati0n you derived in (a)
qsystem = -1834.3J, with a mZn = 34.8g (cZn = 0.390J/goC), What is the ∆T given the heat loss?
111.1Ms = ? ks show work, report sig figs and units
calculate the heat gained by the water: Q=CmΔT heat lost by sample: ms* cs *(Ts-T) = mw *cw (T -Tcw) + mc *cc *(T-Tcw) solve for the specific heat of the unknown known unknown (ms) mass of unknown= 240.40g (Cs) specific heat of sample: ? (Ts) Temp initial of sample: assume 100°C (mc) mass of dry cup: 31.3g (mw) mass of water: 127.3g (cw) specific heat of water: 4186 J/kg °C (Tcw) initial temp of water: 12°C (Cc) specific heat of cup: use Aluminium 900 J/kg °C (T) final temp 23°C (I tried it and I'm not sure if I have a correct answer, so if you can please do it step by step to show me where I made mistakes)
21.7 g of a basic solution was mixed with 87.6 g of water in a calorimeter with a calorimeter constant of 47.6 J K–1 with all substances initially at 29.3 °C.The resulting solution was observed to be at a temperature of 15.4 °C and have a heat capacity of 4.39 J g–1 K–1.Determine q for the mixing process. a. 6670 J b. -1.37 × 105 J c. -7330 J d. -6670 J e. 7330 J
To determine the specific heat of a newly created, highly conducting material, a 704.8 mg sample of the material was supplied with 35.548 J of heat causing the temperature of the material to rise from 297.05 K to 461.4 K. What is the specific heat of this material? Report your answer in units of J/(ºC · g) to 4 sig figs, but do NOT include units in your answer.
a) What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by 0.68 oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) Show your working below:
Nitroglycerin (C3H5N3O9), a liquid at room temperature (25 oC) and atmospheric pressure (1.01325 x 105 Pa) is used to relieve angina. It may undergo decomposition under these same conditions to form nitrogen, carbon dioxide, oxygen and water, with an enthalpy of decomposition of -1541 kJ mol-1The standard enthalpies of formation of water and carbon dioxide are -285.9 kJ mol-1 and -393.5 kJ mol-1 respectively Calculate the work done when 1.0 mole of nitroglycerin decomposes and additionally explain the significance of the sign.
I2(g) + Cl2(g) ⇌ 2 ICl(g) Calculate ΔGrxn in kJ at 25°C from the following ΔG°f values. ΔG°f (I2) = 62.42 kJ/mol ΔG°f (Cl2) = 0 kJ/mol ΔG°f (ICl) = -5.52 kJ/mol Report your answer to 2 decimal places, and do NOT include units.
a) What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by 0.68 oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) b) What is the standard enthalpy of reaction per mole of KOH when 50.00 cm3 of 1.0 moldm-3 of Nitric Acid (HNO3) and 50.00 cm3 of 1.0 moldm-3 of Potassium Hydroxide (KOH) are mixed? According to your simulation, the temperature rose by __6.81__ oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1)
Use the values you measured for Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) ΔH°1: -452kJ, and MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(l) ΔH°2: -133kJ, with the known ΔH°3 = ΔH°f(H2O, l) = –286 kJ/mol, to find your experimental ΔH°f(MgO), as: [f MgO] Mg(s) + ½O2(g) → MgO(s) ΔH°f(MgO) = ΔH°1 – ΔH°2 + ΔH°3 = ______ kJ/mol