A mother solution or a pure can be diluted down to give a lower solution; but you can't dilute down to give a higher concentration, i.e. to go from 30%...
1 Answers 1 viewsAll you have to do here is to convert the mass ratio to a mole ratio by using the conversion factor that takes you from grams to moles or vice...
1 Answers 1 viewsStep 1. Calculate the empirical formula. The empirical formula is the simplest whole-number ratio of atoms in a compound. The ratio of atoms is the same as the ratio of...
1 Answers 1 viewsAs always with these problems, it is useful to assume $100*g$ of unknown compound....and thus find an empirical formula... $"Moles of carbon"=(12.8*g)/(12.011*g*mol^-1)=1.066*mol.$ $"Moles of hydrogen"=(2.1*g)/(1.00794*g*mol^-1)=2.084*mol.$ $"Moles of bromine"=(85.1*g)/(79.90*g*mol^-1)=1.066*mol.$ And we...
1 Answers 1 viewsTo find the percentage of the metal, first determine the difference between the mass of the compound and the mass of chlorine. This will give the mass of the metal....
1 Answers 1 viewsWe can write an equation for the (complete) combustion of the substance as follows: $C_xH_yN_z + (x+y/2+z)/2O_2 to xCO_2+y/2H_2O+zNO_2$ That might look complicated, but all we're saying is that each...
1 Answers 1 viewsIn $100* g$ of this there are $30.4* g$ $N$, and the balance $O$. We divide thru by the atomic masses in order to approach the empirical formula: $(30.4*g)/(14.01*g*mol^-1)$ $=$...
1 Answers 1 viewsYour ultimate goal here is to figure out the smallest whole number ratio that exists between iron and oxygen in this unknown compound, i.e. the empirical formula of the compound....
1 Answers 1 viewsWe must calculate the masses of $"C, H"$, and $"N"$ from the masses of carbon dioxide, water, and nitrogen dioxide. $"Mass of C" = 6.019 color(red)(cancel(color(black)("g CO"_2))) × "12.01 g...
1 Answers 1 viewssince kinetic energy of every gases dipends only from the absolute temperature (Ek = KT) and then at a certain temerature is equal for every gasses, and kinetic energy is...
1 Answers 1 views