Consider the following reaction. How many moles of ethanol (C_2 H_5 O) are requi

Question

Consider the following reaction. How many moles of ethanol (C_2 H_5 O) are required to produce 5.2 moles of CO_2. Assume there is an excess of O_2 present. C_2 H_5 OH(l) + 3 O_2 (g) rightarrow 2 CO_2 (g) 3 H_2 O (g) A. 1.54 moles C_2 H_5 OH B. 3.500 moles C_2 H_5 OH C. 1.83 moles C_2 H_5 OH D. 2.60 moles C_2 H_5 OH E. 6.02 moles C_2 H_5 OH Consider the following balanced reaction. How many grams of iron(III) oxide are required to form 48.05g of H_2 O? Assume that there is an excess of HCl present. The molar masses are as follows: H_2 O = 18.02 g/mol; Fe(OH)_3 = 159.69 g/mol Fe(OH)_3 + 3 HCI rightarrow Fe(CI)_3 + 3 H_2 O A. 174.3 g Fe(OH)_3. B. 53.23 g Fe(OH)_3 C. 266.6 g Fe(OH)_3 D. 141.9 g Fe(OH)_3 E. 79.85 g Fe (OH)3 14. Determine the theoretical yield of HCl if 54.0 g of BCl_3 and 49.5 g of H_2 O are reacted according to the following balanced reaction. Possibly useful molar masses include: BCL_3 = 117.16 g/mol; HCI = 36.46 g/mol; H_2 O = 18.02 g/mol. BCl_3 (g)

Explanation / Answer

Q12

5.2 mol of CO2:

from reaction, we need:

1 mol of ethanol = 2 mol of CO2

so

stoichiometric ratio is 1/2 since 1:2 ratio:

5.2 mol f CO2 = 1/2*5.2 = 2.6 mol of ethanol required

so

choose D

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