Sodium is a metal element. Mass of 3.8 moles is 87.4g.
Sodium reacts with water. 0.652 NaOH moles will form.
7 moles of strontium is equal to 613,34 g.
10,8 g aluminium is equivalent to 0,4 moles.
The answer is 10 moles of carbon monoxide.
2 C + O2 = 2 CO
This reaction emmits H2 gas. We need 7.2 moles of Hcl.
Al+HCl===> AlCl3+H2 Is the reaction. You need &.2 moles of HCl.
The product PV remain constant in a closed system at constant temperature.
750 L hydrogen gas at 0 0C and 1 at is equal to 33,44 moles.
mass/molar mass = moles
This is carbon tetra chloride. there are 0.3636 moles in this mass.
45 g is equal to 1,184 moles fluorine.
20 g anhydrous sodium carbonate is equivalent to 0,188 moles.
This is the general law of gases:
PV = nRT (n is the number of moles)
The pressure is approx. 2 atmospheres.
When there is only one atomic symbol shown for each element in the formula of a compound, as with MgO, the molecular mass is simply the sum of the gramatomic masses, in this instance, 40.304 grams.
Ethane contain 20 % hydrogen.
The reaction is 2HCl(aq) + Mg(s) ==> MgCl2(aq) + H2(g)
3.143 moles HCl will yield 1/2 x 3.143 moles of H2 gas (see balanced equation stoichiometry)
Thus, 3.143 moles/2 = 1.5715 moles H2 gas will be produced
At STP 1 mole - 22.4 liters, thus 1.5715 moles x 22.4 L/mole = 35.20 liters of H2 gas formed
The definition of 0.175 m KF is that 1 kg of water contains 0.175 moles of KF. Thus, 347 g of water is equivalent to 0.347 kg, and to find moles of KF, you calculate as follows:
0.175 moles/Kg x 0.347 kg = 0.0607 moles of KF are present (3 significant figures).
If 3,6 x 10-5 is grams the number of atoms is 1,1.10e17.
The short answer is yes, gas has mass and density. However, you should note that gas is a state of matter, just as solid and liquid are. Since all matter has mass, any substance in its gaseous state has mass. Since all matter occupies space, it has density, since density is defined as mass per unit volume, where volume is space.
Larger objects dont always have more mass than smaller objects.
Sulfur dioxide is SO2, so there are 2 moles of oxygen for each mole of sulfur. In 25 moles of SO2, there are 25 moles of S, so there must be 50 moles of oxygen, or 25 moles of diatomic oxygen gas (O2).
the term gram molecule was used in chemistry and this unit is used to measure a single molecule in gram molecule.
The atomic weight of chlorine (after IUPAC 2009) is [35,446;35,457].
The rounded molar mass is 35,45 g/mol, to 4 significant figures.
So the molar mass of chlorine (Cl2 molecule) will be 70.90 g/mol
It's very easy. First of all we test the given sample in laboratory to know about its constitution. Let's discuss it by taking an example:-
Suppose the constitution of a compound is given as below:-
C = 92.4%, H = 7.6%
let's assume that the sample is 100 gram. so the weight of carbon is 92.4 gram & that of hydrogen is 7.6 gram. Now it's we must make sure that is the total of weights of constituents 100 or not? If it is not 100, it means there is an another element in the compound, and this is always oxygen in case of hydrocarbons.
Step 1st :- Find out the number of moles of each element
number of moles = weight of the element/atomic mass
number of moles of C = 92.4/12 = 7.7 moles
number of moles of H = 7.6/1 = 7.6 mole
Step 2nd:- Find out the relative ratio of the moles:- It is simply done by dividing all by the smallest one
C = 7.7/7.6 = 1.01
H = 7.6/7.6 = 1
Step 3rd:- If the ratio is not whole numbers the multiply all the numbers by a smallest integer number to make them whole numbers.
Here in this case both are nearly whole numbers. so there is need to multiply these numbers.
C = 1
H = 1
Step 4th:- Write the empirical formula
step 5th:- Find the weight of empirical formula
1*12 + 1*1 = 13
now if the molecular weight is given then the molecular formula can be written easily.
molecular weight = ( empirical formula weight)n
for example the molecular weight is 78.
n = 78/13 = 6
so the molecular formula is = C6H6
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