Question

Nitroglycerin, for example, uelu J o (g) 2 CHNO1) -> 6 COB) +3 NG(8) + 5H2O(g) + % If 1.90 g of nitroglycerin explodes, calculate the volume (in liters) that the product gases would occupy if their total pressure is 1.60 atm at 4.95 x10°C. Data: Atomic masses H=1.008, N=14.01, 0= 16.00, C=12.01 Hints: Compute the total number of moles of gases then use the ideal gas equation. Optional Bonus Problem (+4pts) No partial credit. Suppose you are given exactly 1 Liter of a 2.75 x 10' M solution of toluene C.HSCH; dissolved in benzene C.H. Exactly 1 milliliter of this solution is taken and diluted to exactly 1 liter with benzene. Call the resulting solution #2. Next take exactly 1 ml of solution #2 and dilute it to exactly 1 liter with benzene. Call the resulting solution #3. Continue in this manner until you get to solution #8. What is the concentration of solution #8? Calculate the number of molecules of toluene in 1 liter of solution #8. Interpret your result.

Las problem optiona bonus is the one that I requore help with. Thank you

Answer 1

Since on dilution with benzene , the number of millimole of toluene would remains the same . We can apply M1V1 = M2V2

2.75×10^-3M × 1ml = M2×1000ml

M₂ = 2.75×10^-6 M

M2V2 = M3V3

2.75×10^-6×1ml = M3× 1000ml

M₃ = 2.75×10^-9 M

M₄ = 2.75×10^-12 M

M₅ = 2.75×10^-15M

M₆ = 2.75×10^-18M

M₇ = 2.75×10^-21M

M₈ = 2.75×10^-24 M. (Answer)

The number of moles of toluene in 1L solution = 2.75×10^-24mol/L × 1L = 2.75×10^-24mol

The number of molecules of toluene in solution #8 = 2.75×10^-24 × 6.022×10²³

= 1.656 molecules

= 1.66 molecules. (Answer)