Question

46.1 g of ethanol (C2H5OH) is burnt in a rigid 5.00 L container resulting a mixture of gaseous products according to the reaction equation: C2H5OH(g) + 3O2(g) -> 2CO2(g) + 3H2O(g) Calculate the total pressure in the reaction vessel at 200 °C.

(A) 1660 kPa

(B) 3930 kPa

(C) 3.93 x10^6 kPa

(D) 38.8 kPa

(E) 787 kPa

Answer 1

soln 461g of ethanol (C2H5OH) is burnt in a rigid 5.001 container resulting a mixture of gaseous products. Acconding to the reaction : C2H5OHkq) + 30269) — 262c9) +342009) To find - Total pressure in the reaction vessel at 200°C. formula used. PV = nRT R=0.3145 m?Pa.ktimel' n= Totul mol of gas T: Temperature in Kelvin V volume (m3) 16-10-3 m3 51 - 5810-3m3 46.1 mol of C₂H5OH (9) = 46.1 Elmul 200209) + 3H2016). TUNITIE CzH50H (9) + 302 (9) . 1 Initially 2 mal 3 mal finally Total mol of gas = 2+3 T = 5 mol T= 200 + 273.15 = 423.158

Now, PV = nRT Px5610%= 5X0.3145 x 473.15 P = 3934 kPa The total pressure in the reaction vessel at 200'C is 3934 kPa. Therefore auswer (®is consect option ,