5. An unknown organic compound contains 65.44 % C, 5.49 % H, and 29.06 % O by ma

Question

5. An unknown organic compound contains 65.44 % C, 5.49 % H, and 29.06 % O by mass. Its molecular mass is 110 g/mol. What is the molecular formula of the organic compound? If 0.486 g of rhodium(IIl) sulfate reacts with excess sodium hydroxide, what mass of rhodium(lIlD hydroxide may be produced? A 4.00 g sample of AgNO, is reacted with BaClh according to the equation 7. 8. What precipitate forms when aqueous solutions of calcium bromide and potassium phosphate are 9. Which net ionic equation best represents the reaction that occurs when an aqueous solution of 10. Which of the following is described as an oxidation-reduction reaction? 2AgNOs(ay) + BaCh(aq) 2AgCI(s)" Ba(NO2)2(aq) to give 1.85 g of AgCI. What is the percent yield of AgCI? mixed? lithium nitrate is mixed with an aqueous solution of ammonium bromide? a, Al + Fed) Fe + Alt); b. CaO + NaI Cal; + Na20 11. What is the oxidation number of C in Ci2H22O? 12. What mass of Na COs is present in 0.330 L of a 0.125 M Na COs solution? 13. 2KMnOdaq) + 8H:8Odaq) + 5Na2C,01(aq) 2MnSOdaq) + 8H20() + 10000g) + What volume of 0.0123 M KMnOs is required to titrate 0.303 g of Na C:04 dissolved in 30.0 mL of solution? 14. A flexible vessel contains 14 L of gas where the pressure is 0.77 atm. What will the volume be when the pressure is 0.65 atm, the temperature remaining constant? 15. How many moles of gas are in a gas sample occupying 1.67 L at 565 mmHg and 14°C? 16. The density of N2 gas at 8.6°C and 1.45 atm is 17. What is the total volume (L)of gases produced at 712 K and 1.08 atm pressure when 123 g of ammonium nitrite undergoes the following decomposition reaction? NH.NOz(s) Ndg) + 2H20(g) 18. If 79.8 mL of nitrogen gas, measured at 548.4 mmHg and 39.2 °C, reacts with excess iodine according to the following reaction, what mass of nitrogen triiodide is produced? N2(g) +312(s) 2N1(s) 19. Does the following have ground-state noble-gas electron configurations? Mg'" 20. Are the following isoelectronic in their ground-state electron configurations? 21. Is the following isoelectronic with Ne? S and Na Ca2 22. Which of the following species would you expect to have the largest radius? K or Br

Explanation / Answer

Ans 5 :

Let the mass of compound be 100 g

So the mass of C = 65.44 g

H =5.49 g

O = 29.06 g

Number of moles of C= 65.44 / 12.01 = 5.45 mol

H = 5.49 / 1.008 = 5.45 mol

O= 29.06 / 31.999 = 0.908 mol

dividing the number of moles by a common value , we get the ratio as : 1: 1 : 6

So the empirical formula becomes : CHO6

Empirical mass = 12.01 + 1.008 + 6(15.999) = 110 g

dividing molecular mass by empirical = 110 / 110 = 1

So the molecular formula of the compound will be : CHO6

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