Question

In: Chemistry

A 2.95 g sample of an unknown chlorofluorocarbon is decomposed and produces 579 mL of chlorine...

A 2.95 g sample of an unknown chlorofluorocarbon is decomposed and produces 579 mL of chlorine gas at a pressure of 756 Torr and a temperature of 298 K. Part A What is the percent chlorine (by mass) in the unknown chlorofluorocarbon?

Solutions

Expert Solution

Ans. #Step 1: Calculate the moles of chlorine gas (Cl2) using ideal gas equation –

Now, mass of chlorine gas produced = moles x MW = 0.0235 mol x 70.9054 g mol-1

                                                                        = 1.667 g

# Step 2: % Cl2 (wt / wt) = (Mass of Cl2 / Mass of sample) x 100

                                                = (1.667 g / 2.95 g) x 100

                                                = 56.51 %


Related Solutions

1a) A 2.95 g sample of an unknown chlorofluorocarbon (an organic compound containing chlorine and fluorine)...
1a) A 2.95 g sample of an unknown chlorofluorocarbon (an organic compound containing chlorine and fluorine) is decomposed and produces 581 mL of chlorine gas at a pressure of 752 mmHg and a temperature of 298 K. What is the percent by mass of chlorine in the chlorofluorocarbon? 1b) Calculate the density of Freon-11 (CFCl3) at 118 °C and 7.20 atm
A 0.1276 g sample of an unknown monoprotic acid was dissolved in 25.0 mL of water...
A 0.1276 g sample of an unknown monoprotic acid was dissolved in 25.0 mL of water and titrated with 0.0633 M NaOH solution. The volume of base required to bring the solution to the equivalence point was 18.4 mL. (a) Calculate the molar mass of the acid. (b) After 10.0 mL of base had been added during the titration, the pH was determined to be 5.87. What is the Ka of the unknown acid? (10 points)
A 50.67 g sample of an unknown acid requires 25.1 ml of a 0.29 M sodium...
A 50.67 g sample of an unknown acid requires 25.1 ml of a 0.29 M sodium hydroxide solution to reach the point of equal moles. Assuming the acid is monoprotic, what would be the molar mass? what if the acid were diprotic? FIND: molar mass (mono) the molar mass of the unknown acid if monoprotic FIND: molar mass(di) the molar mass of the unknown acid if diprotic
Weight of Unknown #4( in g) Volume of water (in mL) Unknown #4 solution (in g/L)...
Weight of Unknown #4( in g) Volume of water (in mL) Unknown #4 solution (in g/L) 0.118 50.00 2.36 0.127 50.00 2.54 0.112 50.00 2.24 Volume of NaOH used = Final concentration – Initial concentration                                           = 16.49 mL – 4.90 mL = 11.49mL NaOH= 0.01149 L NaOH Exp. # Concentration of NaOH Initial volume of NaOH Final volume of NaOH Volume of NaOH used for titration 1 0.1030M 4.90mL 16.49mL 11.59mL 2 0.1030M 16.49mL 26.01mL 9.52mL 3 0.1030M...
A 9.59 g sample of calcium sulfide was decomposed into its constituent elements, producing 5.33 g...
A 9.59 g sample of calcium sulfide was decomposed into its constituent elements, producing 5.33 g of calcium and 4.26 g of sulfur. Which of the statements are consistent with the law of constant composition (definite proportions)? The mass percentage of calcium plus the mass percentage of sulfur in every sample of calcium sulfide equals 100%. The ratio of calcium to sulfur will vary based on how the sample was prepared. The mass ratio of Ca to S in every...
A 1.00 mL sample of pool "chlorine" (NaClO, density = 1.18g/mL) required 21.12 mL of 0.150...
A 1.00 mL sample of pool "chlorine" (NaClO, density = 1.18g/mL) required 21.12 mL of 0.150 M Na2S2O3 to titrate it to the endpoint using the iodometric technique. What was the molarity and percent of sodium hypochlorite in the pool chlorine?
A 1.912-g sample of calcium chloride is decomposed into its constituent elements and found to contain...
A 1.912-g sample of calcium chloride is decomposed into its constituent elements and found to contain 0.690 g Ca and 1.222 g Cl. Calculate the mass percent composition of Ca and Cl in calcium chloride.
A sample of NaN3(s) fully decomposed into Na(s) and N2(g), and the resulting gas was collected...
A sample of NaN3(s) fully decomposed into Na(s) and N2(g), and the resulting gas was collected over water at 52°C. The collected gas occupied 2.0 L at a pressure of 690 torr. If the vapor pressure of water is 100 torr at 52°C, what mass of NaN3(65.02 g/mol) was reacted? (1) 2.5 g (2) 2.9 g (3) 3.4 g (4) 3.8 g (5) 4.4 g
A 1.000 g sample of copper reacts with an unknown element X to form 1.908 g...
A 1.000 g sample of copper reacts with an unknown element X to form 1.908 g Cu5X9. What is element X??
Suppose that 0.323 g of an unknown sulfate salt is dissolved in 50 mL of water....
Suppose that 0.323 g of an unknown sulfate salt is dissolved in 50 mL of water. The solution is acidified with 6M HCl, heated, and an excess of aqueous BaCl2 is slowly added to the mixture resulting in the formation of a white precipitate. 1. Assuming that 0.433 g of precipitate is recovered calculate the percent by mass of SO4 (2-) in the unknown salt. 2. If it is assumed that the salt is an alkali sulfate determine the identity...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT