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P5.26 A 22.0 g mass of ice at 273 K is added to 136 g of H20() at 310. K at constant pressure. Is...
9. A mass of 35.05 g of H20 (s) at 273 K is dropped into 185 g of H20 l) at 310 Kin an insulated contacting at 1 bar of pressure. Calculate the temperature of the system once equilibrium has been reached. Assume Cp.m for H20 (1) is constant at its values for 298K throughout the temperature range. Given: Cpm(ice) = 75.3 JK-mol-1
25.00 g of steam at 373 K is added to 390 g H2O(l) at 298 K at constant pressure of 1 bar. Is the final state of the system steam or water? Calculate (delta)S for the process. Assume that the final state is liquid water. If this is not the case, the calculated temperature will be greater than 373 K.
A sample of helium behaves as an ideal gas as energy is added by heat at constant pressure from 273 K to 343 K. If 15.0 J of work is done by the gas during this process, what is the mass of helium present? 10064 1× g A sample of helium behaves as an ideal gas as energy is added by heat at constant pressure from 273 K to 343 K. If 15.0 J of work is done by the...
The vapor pressure of ice at 268 K is 3.90 x 10-3 atm and at 273 K, the vapor pressure of ice is 6.00 x 10-3 atm. Calculate the heat of sublimation, ΔHsub of ice in kilojoules per mole.
Help on these would be great! 111) Th of 1 mol of A to B absorbs 15 kcal of heat from the surroundings when it occurs irreversibly. doing no work. At the same T and P, reversible conversion of 1 mol of B to A does 10 kcal of for work done on system, heat absorbed by system.) a) i) For A → B, determine qirrev and wirrev ermodynamics of a Cyclic Process: At 293 K and 1 atm pressure,...
Ice of mass 52.0 g at -10.9° C is added to 220 g of water at 14.8° C in a 111 g glass container of specific heat 0.200 cal/g-°C at an initial temperature of 23.9° C. Find the final temperature of the system. °C
Mass of Styrofoam cups 4.00 g Mass of Styrofoam cups with water 102.30 g Mass of Water 98.3 Initial Temperature of water 22.0 oC Final Temperature 11.4 oC Mass of Styrofoam cups with water plus ice 113.60 g Mass of Iced Added 11.3 g 1. Ice at -10 °C is heated until it becomes liquid water at 10°C. Which heating curve below represents this process? 10| و (2) T T ( °C او ( T (°C) 0 -10 سے ان کا -10...
An ice cube with a mass of 46.4 g at 0.0 ∘C is added to a glass containing 4.20×102 g of water at 45.0 ∘C . Determine the final temperature of the system at equilibrium. The specific heat capacity of water, ?s , is 4.184 J/g⋅∘C , and the standard enthalpy of fusion, Δ?∘fus , of water is 6.01×103 J/mol . Assume that no energy is transferred to or from the surroundings.
An ice cube with a mass of 53.0 g at 0.0 °C is added to a glass containing 368 g of water at 45.0 °C. Determine the final temperature of the system at equilibrium. The specific heat capacity of water, Cs, is 4.184 J/g·°C and the standard enthalpy of fusion, ΔH°fus, of water is 6.01 × 103 J/mol. Assume that no energy is transferred to or from the surroundings.
4. A flask with a volume of 2.20 L, provided with a stopcock, contains ethane gas (C2H6) at a temperature of 310 K and atmospheric pressure 1.013x10 Pa. The molar mass of ethane is 30.1 g/mol. The system is warmed to a temperature of 375 K, with the stopcock open to the atmosphere. The stopcock is then closed, and the flask cooled to its original temperature. A) What is the final pressure of the ethane in the flask? B) Find...