The molar mass of this gas is 92.3 g/mol
Calculation
By use ideal gas equation PV =nRT where
n=mole p=pressure V= volume R = gas constant T= temperature
n = mass /molar mass(MM)
substitute in the equation
PV =(mass/MM)RT
mass = density x volume(V)
Therefore PV =(density xV/ MM) xRT
divide both side by by V
P= (density/Mm) xRT
making MM the subject of the formula
MM = densityPRT
At STP = P= 1 atm, R= 0.0821 L.atm/Mol.k T = 273 K
MM is therefore = 4.12 g/l x 1 atm x 0.081 L.atm/mol.k x 273 K = 92.3 g/mol
The solution for the question above is:
C = 0.270
<span>V = 0.0275L </span>
<span>n = ? </span>
<span>Use the molar formula which is: C = n/V </span>
<span>Re-arrange it to: n = CV </span>
<span>n = (0.270)*(0.0275) </span>
<span>n = 0.007425 mols </span>
<span>(more precise) n = 7.425 x 10^-3 mols
</span>
7.425 x 10^-3 mols is the answer.
Answer:
See explanation
Explanation:
Full molecular equation;
2NH3(aq) + AgNO3(aq) -------> [Ag(NH3)2]NO3(aq)
Full ionic equation
2NH3(aq) + Ag^+(aq) + NO3^-(aq) --------> [Ag(NH3)2]^+(aq) + NO3^-(aq)
Net ionic equation;
2NH3(aq) + Ag^+(aq) --------> [Ag(NH3)2]^+(aq)
When Silver nitrate is mixed with a solution of aqueous ammonia, a white and cloudy solution was observed.
1 is D 2 is c 3 is A and 4 the nucleus is so big because it is one of our largest cells in our body... hope this helps!!!!!!!!!!!
