11.5 g NO2
Molecular mass of nitrogen dioxide, NO2 = 14.0+2(16) = 46.0Amount of NO2 = 25.6/46.0 = 0.557molThere are 0.557 moles of NO2 in a 25.6g sample.
1/2 N2(g) + O2(g) + 33.1 kJ NO2(g)
NO2
in 0.25 moles there are 1.505*10^23 molecules (1 mole of any element=6.023*10^23 molecules)
1 mole NO2 = 46.0055g = 6.022 x 1023 molecules 19.6g NO2 x 6.022 x 1023 molecules/46.0055g = 2.57 x 1023 molecules NO2
Molar mass NO2 = 46.0 g/mole1.18 g NO2 x 1 mol NO2/46.0 g = 0.0257 moles NO2 (to 3 significant figures)
11.5 g NO2
0.41
NO2(g)+SO2(g)-->NO(g)+SO3(g) here NO2 act as a oxidising agent
SO2(g) + NO2(g) ==> SO3(g) + NO(g)Keq = [SO3][NO]/[SO2][NO2] Without knowing concentrations, one cannot calculate the actual value of Keq.
Molecular mass of nitrogen dioxide, NO2 = 14.0+2(16) = 46.0Amount of NO2 = 25.6/46.0 = 0.557molThere are 0.557 moles of NO2 in a 25.6g sample.
The amount of NO2 and SO2 eould
N2O5(g) → 4NO2(g) + O2(g)
SO2(g) + NO2(g) ==> SO3(g) + NO(g)Keq = [SO3][NO]/[SO2][NO2] Without knowing concentrations, one cannot calculate the actual value of Keq.
SO2(g) + NO2(g) ==> SO3(g) + NO(g)Keq = [SO3][NO]/[SO2][NO2] Without knowing concentrations, one cannot calculate the actual value of Keq.
SO2(g) + NO2(g) ==> SO3(g) + NO(g)Keq = [SO3][NO]/[SO2][NO2] Without knowing concentrations, one cannot calculate the actual value of Keq.