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The volume of a sample of ideal gas at 25 degrees celius is 372 mL. what will be the volume of the gas if it is heated at constant pressure to 50 degrees celius? what will the volume fo the gas be if it is cooled to -272 degrees celius.
How much would an empty volumetric flask, (weighing 27.16 grams, has a volume of 100.4 cm3 ) weigh when filled with bromine, an element that has a density of 3.1028 g/cm3.
Calculate the final temperature when a 16.4 gram sample of ice at 0oC is placed into a styrofoam cup containing 126 grams of water at 72.7 oC. Assume that there is no loss or gain of heat from the surroundings.
How many grams of sucrose must be added to 552g of water to give a solution with a vapor pressure 2.o mmHg less than that of pure water at 20 celsius?
The moles of salicylic acid is 0.00724mol. The molar mass is 138.12 salicylic acid . Given 1.00 g of salicylic acid . Please show work? m=mol of solute X particles per formation/ mass of solvent, kg
the temperature of a 4.00L sample of gas is changed from 10.0c to 20.0c. what will the volume of this gas be at the new temperature if the pressure is held constant?
If a gas held at constant pressure had an initial volume of 5.00 L and the temperature changed from 35°C to 578 K what would be the final volume of this gas?
The specific heat of Ti is .523 J/gcelcius. What is the final temperature of 62g of Ti intially at 41celcius after 8.5kj of heat is added?
A 29.0-g sample of water at 260. K is mixed with 51.0 g water at 340. K. Calculate the final temperature of the mixture assuming no heat loss to the surroundings.
When a container is filled with 3.00 mol of H2 , 2.00 mol of O2 , and 1.00 mol of N2 , the pressure in the container is 465 kPa. The partial pressure of O2 is ?
Calculate the amount of heat [kcal] released when 50.0 g of steam at 100 °C hits the skin, condenses, and cools to a body temperature of 37 °C.
The temperature of a 35.2 g sample of iron increases from 23.7 C to 29.5 C. If the specific heat of iron is 0.450 J/g-K, how many joules of heat are absorbed.
Consider an experimental run at 273k where the initial number of moles is actually 1.00 , and the final number of moles is 2.00 . Use the simulation to find the volume of 1.00 of helium at 273k and calculate the final volume.
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