Hydroxyl ammonium nitrate contains 29.17 mass % N, 4.20 mass %H, and 66.63 mass

Question

Hydroxyl ammonium nitrate contains 29.17 mass % N, 4.20 mass %H, and 66.63 mass O. If its molar mass is between 94 and 98 g/mol, what is its molecular formula? A) N_2H_4O_4 B) N_3H_3O_3 C) N_2H_2O_4 D) N_4H_8_O_2 E)NH_2O_5 What is the [H^+] in a solution with a pH of 5.63? A) 2.3 times 10^-6 MH^+ B) 2.344 times 10^-6 MH^+ C) 2.3 times 10^-5MH^+ D) 2.344 times 10^-5MH^+ E) 5.63M H^+ During a titration, it is found that 53.5 mL of a solution of NaOH is needed to neutralize a solution that contains 1.86 g of HCl. What is the concentration of the NaOH solution? NaOH (aq) + HCl (aq) rightarrow NaCl (aq) + H_2O (l) A) 1.05 M B) 0.953 M C) 0.686 M D) 0.051 M E) 0.035 M Which of these compounds is a weak electrolyte? A) KCl B) NH_3 C) N_2 D) HCl E) C_6H_12O_6 (glucose) A system delivers 1275 J of heat while the surroundings perform 854J of work on it. What is delta U of the system? A) -2129 J B) +2129 J C) +421 J D) -421 J E) -1275 J

Explanation / Answer

Ans 26 A. N2H4O4

let the mass of compound be 100 g

29.17 % of nitrogen will be 29.17 g = 29.17 / 14 = 2.08 moles

4.20 % of hydrogen will be 4.20 g = 4.20 / 1 = 4.20 moles

66.63% of oxygen will be 66.63 g = 66.63 / 16 = 4.16 moles

dividing all the moles with a common factor 2.1 we get the empirical formula as NH2O2

the empirical formula mass will be 14 + (2 x1) + (2 x 16) = 48.

this almost the double of molar mass

so multiply this empirical formula with 2 to get the molecular formula

So the molecular formula comes out to be N2H4O4

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