Two flasks of equal volume and at the same temperature contain different gases.?
One flask contains 5.0 g of O2, and the other flask contains 5.0 g of H2. Is each of the following statements true or false? Explain. The pressures in the flasks are the same. 1) True. Because the gases have the same mass, they exert the same pressures. 2) True. Both the volumes and the temperatures of the gases are the same, which means that their pressures must be equal. 3) False. There are different numbers of moles in the flasks, meaning that the pressures are different.
Two gases have same volume, pressure and temp. Which container weighs more? 02 and N2?
well the relative atomic mass of 02 is greater the that of N2 so i would say.. 3. the container of oxygen
3 identical containers are at the same temperature, pressure, volume and have the same amount of moles. One container is filled with...?
3 identical containers are at the same temperature, pressure, volume and have the same amount of moles (7.5 mol of each gas per container). One container is filled with Nitrogen gas (N2), the other with Chlorine gas (Cl2), the final one with Argon gas (Ar). Which container has the highest pressure? Use kinetic molecular theory to prove your answer.
Equal volumes of SO2(g) and NO(g) at the same temperature and pressure would have the same?
the only correct answer here is "D" ******************* PV = nRT n = PV/RT.. if P, V, R, and T are constant so are moles...n... as to the other answers. mass = moles / mw.. mw SO3 = 64g/mole.. mw NO = 30 g/mole...so same # moles gives different mass there are 3 atoms in 1 molecule of SO2 so there are 3 moles of atoms in 1 mole of SO2... there are 2 atoms in 1 molecule of NO, so there are 2 moles of atoms in 1 mole of NO...so there would be 50% more atoms in the SO2 than in the NO. density = mass / V... different mass same volume gives different density...
Why is specific heat at constant pressure greater than specific heat at constant volume?
When a gas is heated at const vol., no external work is done and so the heat supplied is consumed only in increasing the internal energy of gas. But if the gas is heated at constant pressure, the gas expands against pressure so does some external work. In this case the heat supplied is used up in increasing the internal energy of gas and in doing some external work.since the internal energy depends only on the temp., so for the same value of temp the internal energy of gas will increase by same amount whether the pressure and vol remains constant. But since ext. work is additionally done for cont. pressure process. So for same rise of temp. more amount of heat is supplied at const. pressure thats why specific heat at const. pressure is greater than specific heat at const. vol..
If two containers have helium and oxygen at the same temperature, pressure and volume, will they have same heat capacities?
Heat capacity depends on specific heat of the material. And specific heat is an intensive property (independent of mass of the system). Thus, heat capacity will be different for both systems.
If the volume is the same will the mass be the same?
Only for the same element/alloy/substance with exactly the same density, which can mean the same temperature and pressure too.
Chem - Volume -EASY BEST ANSWER?
1. 1 mole of neon occupies 22.4l 8 mole of neon occupies 22.4*8l=179.2l 2. First find out the volume of oxygen required as:- 1 CH4 + 2 O2 -> 1 CO2 + 2 H2O 1 mole of methane requires 2 moles of oxygen 22.4 l of methane requires 44.8 l of oxygen 2 l of methane requires 4 l of oxygen Now convert it to the required temp.and pressure gas equation. It comes out to be 2.183150 l or 2.2 l approximately 3. CO2 produced at s.t.p. is 2 l Now convert it to the required temp.and pressure gas equation. It comes out to be 0.219780 l or 0.2 l approximately That's it ans-1 179.2 l ans-2 1.1 l ans-3 0.2 l
Chem help what is the volume of this gas at the same temp and pressure?
0.820 mole of hydrogen gas has a volume of 2.00 L at a certain temperature and pressure. What is the volume of 0.125 mol of this gas at the same temperature and pressure