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how many ml of water at 10 degrees celsius (2 significant figures) must be added to 75 ml of water at 35 degrees celsius to obtain a final temperature of 19 degrees celsius?
Q=mCΔT ; where m is the mass of the substance, C is the specific heat of the substance, and ΔT is the difference in temperature.35 -19 = 1619-10 = 916...
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What phase changes, if any, occur if carbon dioxide initially at -80 degrees celsius and 8.0 atm is allowed to warm to -25 degrees celsius at 5.0 atm?
Using law PV = nRT, you can see, that if n,R = const, and T and P are used for some processes,V-volume is the one,that can be changed.
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Calculate q, w, delta E and delta H for the process in which 2.0 moles of N2O gas are cooled from 165 degrees Celsius to 55 degrees Celsius at a constant pressure of 5 atm.
delta E=0 delta H = Cp delta T delta U = Cv delta T + p delta V q = delta H w = p delta V delta U =...
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If the total air pressure is 1.05 atm, the partial pressure of carbon dioxide is 0.08 atm, and the partial pressure of hydrogen sulfide is 0.05 atm, what is the partial pressure of the remaining air?
As we know, Total pressure is the sum of partial pressure of individual gases.PT = 1.05 -(0.08+0.05+Pair)Pair = [0.92] atm
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Determine the new volume of a gas at that occpies an original volume of 55 L at 750mmHg and 25 degrees celsius if the pressure is changed to 1.03 atm and the temperature to 30 degrees celsius.
According to the ideal gas equation:P1V1/T1 = P2V2/T2,where P1, V1, T2 - initial pressure, volume and temperature, P2, V2, T2 - pressure, volume and temperatureAs a result:V2 = P1V1T2 /...
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A sample of an ideal gas has a volume of 3.60 L at 13.40 degrees Celsius and 1.30 atm. What is the volume of gas at 24.60 degrees Celsius and 0.990 atm
Combined gas Law P1V1 / T1 = P2V2 / T2 P1 = 1.30 atm V1 = 3.60 L T1 (must be in Kelvin = 13.40 deg C + 273.15) =...
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If a gas is at 1.2atm, 25 degrees Celsius, and 10 liters what is the new volume if the pressure is changed to 2.8atm and the temperature to 35 degrees Celsius?
4.43 litersThe general gas equation :P1V1/T1 = P2V2/T2. Where p1=1.2atm; V1= 10 litersT1= 273 + 25=298 KP2=2.8 atmT2= 273+35=308 KV2 - ?V2=(p1*V1*T2)/(T1*p2) ;V2= 4,43 liters
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A helium balloon occupies 112mL at 90.0 kPa and 34 degrees Celsius. What volume would it occupy at standard temperature and pressure (101.3 kPa 0.00 degrees Celsius)
Use the combined gas law.P1V1/T1 = P2V2/T290*0.112/307 = 101.3*V2/2730.0328 = 0.3711*V2V2 = 0.088L
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The volume of a gas is18.4 ml at 24.0 degrees Celsius. What will the volume be at 12.0 degrees Celsius and 0.889 atm?
P1*V1/T1 = P2*V2/T2V2 = T2*V1/T1 = 285K*0.0184L/297K = 0.01766 L
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a 275L helium balloon is heated from 20 degrees celsius to 40 degrees celsius. what is the final volume at constant pressure?
pV=nRT.VxT2/T1= 275 x 40/20 = 550.
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