A compound is found to be 30.45% N and 69.55% O by mass. If 1.63g of this compound occupies 389 mL at 0.00 degrees Celcius and 775 mmHg, what is the molecular formula of the compound.
I know I need to convert those numbers so they can fit into the Ideal Gas law, I just don't know where to go from there.
I know I need to convert those numbers so they can fit into the Ideal Gas law, I just don't know where to go from there.
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1. Find the mass of each element and convert to moles
nitrogen: (1.63 g x 0.3045) / 14.0 g/mol = x
oxygen: (1.63 g x 0.6955) / 16.0 g/mol = y
2. Find the simplest ratio of x to y to get the empirical formula of compound ( NxOy)
3. Find molar mass of empirical compound
4. Use ideal gas law to find moles (n) of compound n = PV/RT
5. Find molar mass of compound (1.63 g/ n = )
6. Divide molar mass by empirical molar mass to find factor with which to multiply subscripts of empirical formula to get formula of compound
nitrogen: (1.63 g x 0.3045) / 14.0 g/mol = x
oxygen: (1.63 g x 0.6955) / 16.0 g/mol = y
2. Find the simplest ratio of x to y to get the empirical formula of compound ( NxOy)
3. Find molar mass of empirical compound
4. Use ideal gas law to find moles (n) of compound n = PV/RT
5. Find molar mass of compound (1.63 g/ n = )
6. Divide molar mass by empirical molar mass to find factor with which to multiply subscripts of empirical formula to get formula of compound
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whoh! too much sciencey stuff! Im just gonna chill and do some biology...