るH219)さN2(g) >2Hg( Heat How is equilibnum affecteedby an creasein Rssue けでうow A) cannot be determined ups tro B) it shiftS to the left 02 c)if shifts to the right D)it has no effect 29How is equilibnumaffected by a decrease in temperature? son A)エ+ shこfts to the lef B)E c)エキ shifts to the ng nt D)cannot be determined. It has no effect

54.73 g of water, H2O, 18.02 g/mol, was heated from -19.53 °C to 112.08 °C.  The freezing and boiling point of water is 0.0 °C and 100. °C, respectively. The specific heat capacities of solid, liquid, and gaseous water is 2.03 J/(g*K), 4.18 J/(g*K), and 1.84 J/(g*K), respectively. The heat of fusion and vaporization of water is 6.01 kJ/mol and 40.67 kJ/mol, respectively. How much heat, in kJ, is required?

12. Match the name to the organic compound 1 H CEC -H A. ethane B. ethene H-C-C H. C. ethyne H-C-C OH H H нн D. ethanal Н-С-С-О-С-С-н H H нн нн E. ethanoic acid H-C-C-H H H H. F. ethanone 6. C=C H. H. G. diethyl ether H. ethanol H. HICIHHI 2. 3.

altcal 54cal Part A 25 of 27 How much heat in kilocalories is required to melt 3.0 mol of isopropyl alcohol (rubbing alcohol; molar mass 60.0 g/mol)? The heat of fusion and heat of vaporization of isopropyl alcohol are 21.4 cal/g and 159 cal/g, respectively VAED 3.0 mol bo.0g ? mo kcal Submit Request Answer Part B How much heat in kilocalories is required to vaporize 3.0 mol? ? VAXp kcal

How much energy is evolved when 100g ofwater loses 15c temperature. The specific heat of water is 4.184J/gC? 350J   +6.2KJ   -6.2KJ   You can't tell because you don't know either the starting or the end temperature.

If the  ∆Hcomb of C4H10 = -2871 kJ/mol.  What would be the final temperature of 850.0 mL of water at 24.0oC if it absorbed the energy from the combustion of 4.5 grams of C4H10? Your Answer should follow the format: a) mols of C4H10 b) energy change (q) of water with units  c) ∆t of water d) final temperature of water

Is the following process exothermic or endothermic?   2H(g) ⟶⟶ H2(g)

H8. The enthalpy of vaporization of benzene, C6H6(l) is 33.9 kJ/mol at 298 K. How many liters of C6H6(g), measured at 298 K and 95.1 mm Hg are formed when 1540 J is absorbed by, C6H6(l) at a constant temperature of 298 K? (Anwser in L) How do you work this problem out correctly using Clausius-Clapeyron Equation?

7:02 AM Wed Feb 1 Question 14.c of 26 Consider the heating curve provided for 1.00 mole of a substance that begins as a solid at -14.8 °C and ends as a gas at 121.1 °C. Specific heat capacities: solid = 145.6 J/ mol °C, liquid=97.25 J/mol °C, gas = 68.49 J/mol. °C Step C: What quantity of heat energy (in kJ) must be absorbed to increase the temperature of the liquid from the melting temperature to the boiling temperature? Learn More in OpenStax

BH3 A0 kMno, Naolt, Hao Heat G HBr AIBU Heat Nalt Mc PB A 464