Mass of carbon = 0.1927 g
Mass of hydrogen = 0.02590 g
Mass of nitrogen = 0.1124 g
Mass of phosphorus = 0.1491 g
Mass of Oxygen = 0.8138 - ( 0.1927 + 0.02590 + 0.1124 + 0.1491 ) = 0.3337 g
Moles of C = [tex]\frac{0.1927}{12.011} = 0.0160 mol[/tex]
Moles of H = [tex]\frac{0.02590}{1.008} = 0.0257[/tex] mol
Moles of O = [tex]\frac{0.3337}{15.999} = 0.0209 mol[/tex]
Moles of P = [tex]\frac{0.1491}{30.974} = 0.00481 mol[/tex]
Moles of N = [tex]\frac{0.1124}{14.01} = 0.00802 mol[/tex]
So, the empirical formula will be: [tex]C_{0.0160} H_{0.0257} O_{0.0209} N_{0.00802} P_{0.00481}[/tex]
To make it a whole divide the moles of all elements by 0.00481.
Therefore, [tex]C_3_3 H_5_5 O_4_3 N_1_7P_1[/tex].
Molecular mass of ATP = 507 g/mol
Empirical formula = 164.063 g/mol
Molecular formula:
[tex]\frac{507}{164} = 3[/tex]
So, molecular formula is [tex](C_3_3 H_5_5 O_4_3 N_1_7P_1)_3[/tex] = [tex]C_1_0 H_1_6 O_1_3 N_5P_3[/tex]
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