Propane (C_3H_3) burns in oxygen to produce carbon dioxide gas and water vapor.

Question

Propane (C_3H_3) burns in oxygen to produce carbon dioxide gas and water vapor. Write a balanced equation for this reaction. Calculate the number of liters of carbon dioxide measured at STP that could be produced from 7 45 g of propane. Chlorine gas was first prepared in 1774 by the oxidation of NaCl with MnO_2: 2 NaCI(s) + 2H_2SO_4(l) + MnO_2(s) rightarrow Na_2SO_4(s) + MnSO_4(s) + 2 H_2O(g) + Cl_2(g) Assume that the gas produced is saturated with water vapor at a partial pressure of 28.7 mmHg and that it has a volume of 0.597 L at 27 degree C and 755 mmHg pressure. What is the mole fraction of Cl_2 in the gas? How many grams of NaCI were used In the experiment, assuming complete reaction? A gas mixture for use In some lasers contains 5.00% by weight HC1, 1.00% H_2, and 94% Ne. The mixture is sold in cylinders that have a volume of 49.0 L and a pressure of 13,800 kPa at 21.0 degree C. What is the partial pressure in kilopascals of each gas in the mixture?

Explanation / Answer

prob 9)

a) C3H8 + 5O2 --------> 3CO2 +4 H2O + heat

b) from balence chemical equation one mol of propane react with 5 mol of O2 to produce 3 mol of CO2 and 4 mol of H2O

number of moles of propane = (7.45 g / 44g/mol) = 0.17 mol

mol of CO2 = 3*0.17 = 0.51 mol

mass of CO2 = (44g/mol * 0.17 mol) = 7.45 g

One mole of an ideal gas will occupy a volume of 22.4 liters at STP (Standard Temperature and Pressure, 0°C and one atmosphere pressure).

so volume of CO2 = (22.4 L *0.51 mol) = 11.424 L

prob 10)

a) mol fraction of Cl2 = partial pressure Cl2 / total pressure

mol fraction of Cl2 = (28.7mmhg / 755mmhg) = 0.038

b) PV = nRT

n = (0.0375atm x 0.597 L) / (0.082 atm.L/K.mol x 300K) = 0.91 moles

from balence chemical reaction 2 mol of NaCl produce 1 mol of Cl2 ratio is 2:1

so number of mol of NaCl = 0.91 x 2 =1.82 moles

mass of NaCl = (1.82 mol x 58.45 g/mol) 106.38 g

prob (11) let 100 g solution then HCl = 5g,H2=1g,Ne=94g

moles of HCl = (5/36.5) =0.137 moles,

moles of H2 = (1/2) = 0.5 moles

moles of Ne = (94/20.18) = 4.658 moles

mol fraction of HCl= 0.137/5.296 = 0.0258 H2 = 0.0944, Ne = 0.88

partial pressure of HCl =0.0258 x 13800 Kpa = 356 Kpa

partial pressure of H2 = 0.0944 x 13800 Kpa = 1302.7 Kpa

partial pressure of Ne = 0.88 x 13800 kpa = 12137.5 Kpa

Related Questions

Navigate

• Browse (All)
• Browse P
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.