11)MM of ccl4=12+142=154
no of moles of atoms =1025/NA
no of moles of molecules=1/5*1025/NA
mass of ccl4=no of moles of ccl4 * MM
volume of ccl4=mass/density=1/5*1025/NA
* MM1.5gm cm-3
Two jars A and B of equal capacity contain 10g of oxygen and 10g ozone respectively.Is the number of molecules equal in both jars?Which jar has greater number of atoms?Write the equation governing both parts or find the anomaly with regard to the avogadros law "equal volumes of gases contain equal number of molecules "
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1There is a correction in the 4 th question :
If side of the cubical container is 2.82 dm ... assume the density of water vapour to be β .... mass of water vapour = 18 gm and STP condition holds.
What is the volume of the water vapour in the container?
1sharad , khyati your answers are correct ...
now attempt the 4 th question
12)its easy....here the gas is in NTP.we know that the mass of 22.4 L of any gas at NTP is equal to its molar mass.
so mloar mass is=22.4*1.5=33.6gm.
1@qwerty,unless otherwise stated i think it is generally assumed that the gases are in NTP
11Ans 3) density = 0.999841 at 273 K
density = mass/volume
put the values, mass = 18g
answer is 18.00286246ml.
The volume occupied by one mole of substance is called the molar volume. The molar volume of liquid water is 18.016/density. At 277 K, the molar volume is 18.016 mL. For liquid water, the molar volumes of liquid water increase to 18.03 mL at both 269 K and 285 K.
1HI PRATEEK
SEE AVAGARDO LAW STATES THAT' EQUAL VOLUMES OF DIFFERENT GASES UNDER SIMILAR CONDITIONS OF TEMP. AND PRESSURE CONTAINS EQUAL NO OF MOLECULES'
U HAVE NOT SPECIFIED THE CONDITIONS.'
1Try these questions it is similar to the kind of questions where we feel that the question is incomplete but actually it is not ::
1) What volume of carbon tetra cholride CCl4 having density 1.5gm cm-3 contains 10 25 atoms ?
2) What is the molar mass of a gas if 1.00 L of the gas weighs 1.50 gm at 273 K and one atmospheric pressure ?
3) What is the molar volume of water at 273 K ? Density of water is 1gmcm-3.
4) What is the volume of water vapour in a container , where the side of cubical container is 22.4 dm and the mass of water vapour is 18 gm and the conditions are STP.
1sharad u are correct (i did not want to change the question because nowhere it was mentioned that the conditions are same)....it is given that the mass is same for both the gases (and they are not at STP) obviously i did not know this earlier that unless it is mentioned we cannot use the STP CONDITION
11yeh same no of atoms too.( sorry woh post galti se delete ho gaya, I was just going to click on edit aur delete par kar diya)
any ways thanks.
1@ prateek ,avogadros law states "equal volumes of gases contain equal number of molecules ".
here,the mass of both gases is the same,but not the volume.so they will contain unequal no of molecules.
no of moles of oxygen gas will be =10/32 and ozone will be=10/48.
no. of atoms of oxygen gas will be=10/32*2*NA and in ozone it will be=10/48*3*NA
so both contain equal no of atoms.......
23@ prateek how can we assumethe conditions of pressure and temperatue ?? these functions depend on the gas itself . If both ozone and oxygen were in identical jars , den they will hav equal no of molecules or moles only if they would hav exerted same pressure at same temperature....the converse is also true
if they would hav exerted same pressure at same temp in 2 identical jars, then only they would hav equal no of moles
71No they aren't same... Weights are different and Avogardo's law says for VOlumes!
1Do we measure the gases in terms of weight or volume?
Cuz in the question when you say 10gm of Oxygen or 20gm of Ozone, what does that mean? Is it appropriate to calculate in terms of weight?
If so, then our answer is easy:-
n= weight of sub./ gm.mol. wt.
That means simply calculate the no.of moles and then from the formula of N=6.023*(10^23)*n calculate the no.of molecules.
where N is the no.of molecules and n is the no.of moles.
1they are same for both.. bcoz it is not mentioned in the question..