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An ideal gas starts with a pressure of 0.980 atm and a temperature of 23oC. The pressure raises to 1.1 atm. What is the new temperature of the gas?
P1/T1 = P2/T2T2 = P2 x T1 / p1 = 1.1atm x 300k / 0.980atm = 336.7k = 63.7oC
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1. Ninety five percent (95%) of solute is removed from 150 mL of an aqueous solution by extraction with 20 mL of an organic solvent. What is distribution ratio of the solute?
95% of 150 ml is 142.5 mLDistribution coefficient = (volume is aqueous layer/volume is organic layer)= 142.5/20 = 7.125
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25.0 g of an unknown metal at 90.0C is added to 50.0 g of water at 25.0 oC causing the temperature of the water rises to 29.8oC. What is the specific heat capacity and the identity of the metal?
qmetal = qwater By substitution, we have (metal values on the left, water values on the right): (mass) (Delta;T) (Cp) = (mass) (Delta;T) (Cp) (25.0)(90-29.8)(Cp) = (50.0)(29.8-25.0)(4.184 J g-1...
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Calculate the amount of heat required to heat a 3.1 kg gold bar from 25 ∘C to 69 ∘C. Specific heat capacity of gold is 0.128 J/g∘C
Q = c*m*ΔT = 0.128*3100*(69-25) = 17459 (J) = 17.5 (kJ)
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mass of acetic acid?
molar mass=60.052 g/mol
heat capacity=8.43kj/C
temp increase from 24.5 C to 36.8 C
deltarU for combustion =-874.2kj/mol
Answer on Question #83705, Chemistry/ Organic Chemistrymass of acetic acid?molar mass=60.052 g/molheat capacity=8.43kj/Ctemp increase from 24.5 C to 36.8 CdeltarU for combustion =-874.2kj/molSolution:ΔErxn = qrxn = -qcal = -Ccal*Δt =...
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Define heat capacity; molar heat capacity and specific heat capacity of a substance and give relations between them.
Heat capacity or thermal capacity is a physical property of matter, defined as the amount of heat to be supplied to a given mass of a material to produce a...
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A 126 piece of metal is heated to 285 and dropped into 83.0 of water at 26. If the final temperature of the water and metal is 58.3, what is the specific heat of the metal ?
Q = c*m*(t2-t1) Q(metal) = Q(H2O) Q(H2O) = c(H2O)*m(H2O)*(t2(H2O) ndash; t1(H2O)) = 4.186 * 83 * (58.3 ndash; 26)= 11.2 kJ Q(metal) = c(metal)*m(metal)*(t1(metal) ndash; t2(metal)) = c(metal) * 126...
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115.24g of isopropyl alcohol at 20.1 degrees is mixed with 56.31g of water at 50.3 degrees after thermal equilibrium was reached, the temp was 36.5, what was the energy lost by water
Q = C x m x deltaTCwater = 4200 J/kg°CQ = 4200 x 0.05631 x (50.3 - 36.5) = 3264 J
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A certain calorimeter absorbs 65 J/oC. If 55.0 g of 67oC water is mixed with the calorimeter’s original 50.0 g of 23oC water. Calculate for the final temperature of the mixture?
Q = C x m x deltaTCwater = 4.186 J/g°CQ1 = 4.186 x 55 x 67 = 15 425 JQ2 = 4.186 x 50 x 23 = 4 814 JQ3...
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What amount of heat is required to convert 1.0 g of water at 67.0°C to 1.0 g of steam at 100.0°C? (heat capacity of water = 4.184 J/g • C; ∆Hvap = 40.7 kJ/mol)
Q= Q1 + Q2Q1 = cm(T2 - T1) =4.184 *1.0*(100-67)= 138.072 JQ2= ∆Hvap*nn = m/M = 1.0 / 18.02 = 0.055 molQ2= 40700J /mol * 0.055 mol = 2239 JQ...
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