How many grams are there in 7.4 x 1023 molecules of H2SO4?

Chemistry

1 answer:

bazaltina [42]3 years ago

4 0

7.4x10^23 = molecules of silver nitrate sample

6.022x10^23 number of molecules per mole (Avogadro's number)

Divide molecules of AgNO3 by # of molecules per mol

7.4/6.022 = 1.229 mols AgNO3 (Sig Figs would put this at 1.3)

(I leave off the x10^23 because they both will divide out)

Use your periodic table to find the molar weight of silver nitrate.

107.868(Ag) + 14(N) + 3(16[O]) = 169.868g/mol AgNO3

Now multiply your moles of AgNO3 with your molar weight of AgNO3

1.229mol x 169.868g/mol = 208.767g AgNO3

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For the reaction below, complete the rate expression that relates the change in concentration with respect to time to the rate o

Ann [662]

Answer: Rate in terms of disappearance of $NO$ = $-\frac{1d[NO]}{2dt}$

Rate in terms of disappearance of $Cl_2$ = $-\frac{1d[Cl_2]}{1dt}$

Rate in terms of appearance of $NOCl$ = $\frac{1d[NOCl]}{2dt}$

Explanation:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

$2NO+Cl_2\rightarrow 2NOCl$

The rate in terms of reactants is given as negative as the concentration of reactants is decreasing with time whereas the rate in terms of products is given as positive as the concentration of products is increasing with time.

Rate in terms of disappearance of = $-\frac{1d[NO]}{2dt}$

Rate in terms of disappearance of = $-\frac{1d[Cl_2]}{1dt}$

Rate in terms of appearance of $NOCl$ = $+\frac{1d[NOCl]}{2dt}$