well since it getting to old were using a new system because we are flammers
One unit of dinitrogen tetraoxide gas is decomposing into two units of nitrogen dioxide gas.
One unit of dinitrogen tetraoxide gas is decomposing into two units of nitrogen dioxide gas.
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)
The chemical formula for that reaction is 2n2o5 -->2 no2+3o2. It describes the process of two distinct compounds coming together to form two new ones.
The question, "translated" into arithmetic, is, "what is the value of the fraction: [76.3 g/(92.02 g/mole)], and the answer is 0.800 moles, to the justified number of significant digits.
One unit of dinitrogen tetraoxide gas is decomposing into two units of nitrogen dioxide gas.
One unit of dinitrogen tetraoxide gas is decomposing into two units of nitrogen dioxide gas.
The empirical mass of NO is 14 + 16 = 30 Divide 138 / 30 ~ = 4.5. The fact that the numbers are not whole number would suggest that the empirical formula is incorrect. However, if we use say NO2 as the empirical formula , then the empirical mass is 14 + 16 + 16 = 46 divide 138 /46 = 3 So NO2 has a formula of N3O6 . This substance does not exist, So it would suggest that the formula is 3NO2 (3/2)N2O4 . I would suggest that the original empirical formula is incorrect. and that the substance is either nitrogen dioxide (NO2) or dinitrogen tetroxide N2O4.
1/2 N2(g) + O2(g) + 33.1 kJ NO2(g)
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)
The chemical formula for that reaction is 2n2o5 -->2 no2+3o2. It describes the process of two distinct compounds coming together to form two new ones.
The question, "translated" into arithmetic, is, "what is the value of the fraction: [76.3 g/(92.02 g/mole)], and the answer is 0.800 moles, to the justified number of significant digits.
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
SO2(g) + NO2(g) ==> SO3(g) + NO(g)Keq = [SO3][NO]/[SO2][NO2] Without knowing concentrations, one cannot calculate the actual value of Keq.