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Consider the following unbalanced chemical equation for the combustion of pentane C5H12

C5H12 (l) O2 (g)  CO2 (g) H2O (l) 

If 20.4 g of pentane are burned in excess oxygen, what mass of water can be produced, assuming 100% yield?

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Neal Broomhead
Neal BroomheadLv7
15 Nov 2020

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Related questions

Question 20 (10 points) Question 20 Unsaved What volume of water vapor could be generated at 1.00 atm and 450. K by the combustion of 250. grams of pentane (C5H12) with 750. grams of oxygen gas? Given: C5H12(g) + 8 O2(g) ---> 5 CO2(g) + 6 H2O(g) Hint: What is the limiting reagent?

Given the heat of combustion for the following reactions, determinethe enthalpy of formation for pentane, C5H12.

C5H12 (l) + 8O2 (g) ----> 5CO2 (g) + 6H2O (l)
Delta H = -3505.8 kJ/mol

C (s) + O2 (g) -----> CO2 (g)
Delta H = -393.5 kJ/mol

H2 (g) + (1/2)O2 (g) ------> H2O (l)
Delta H = -286 kJ/mol

Possible answers:
a. +35 kJ/mol
b. + 1,073 kJ/mol
c. -4,185 kJ/mol
d. -2,826 kJ/mol
e. -178 kJ/mol

Part A For which of the following reactions is ?H?rxn equal to ?H?f of the product(s)? Check all that apply.

Li(s)+12F2(l)?LiF(s)

S(s)+O2(g)?SO2(g)

SO3(g)?12O2(g)+SO2(g)

SO(g)+12O2(g)?SO2(g)

Li(s)+12F2(g)?LiF(s)

2Li(s)+F2(g)?2LiF(s)

Part B The combustion of pentane, C5H12, occurs via the reaction C5H12(g)+8O2(g)?5CO2(g)+6H2O(g) with heat of formation values given by the following table: Calculate the enthalpy for the combustion of pentane. Express your answer to four significant figures and include the appropriate units. ?H?rxn =___value___ ____units___

Substance ?H?f
(kJ/mol)
C5H12 (g) -119.9
CO2(g) ?393.5
H2O(g) ?241.8

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