Question

Propane gas (CH), a fuel for camp stoves, reacts with O, to produce Co, and H,0. a) Write the equation for this reaction. Balance the equation. b) What type of reaction is this? c) How many moles of Co, will be produced from 35.8 moles of O2 d) How many grams of O2 are required to react with 22.0 g of C,H,

Answer 1

Hi there,

(a) The Balanced equation: C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (g)

because huge amount of heat energy released during the course of reaction, hence water is also in gaseous state

(b) This is combustion reaction type

(c) from above balanced equation we know 5 moles O2 gives 3 moles CO2, in other words 1 mole O2 gives (3/5) moles CO2. Hence 35.8 moles O2 can produce = 35.8 x (3/5) = 21.48 moles CO2

Answer: 21.48 moles of CO2 will be produced

(d) moles C3H8 in 22.0 g = 22.0 g / 44.1 g/mol = 0.49886621315 moles

moles O2 required = 5 x 0.49886621315 = 2.49433106576 moles O2 required

mass O2 required in grams = 2.49433106576 mol x 31.9988 g/mol = 79.8156 g

Answer: grams of O2 required = 79.8 grams

Hope this helped you!

Thank You So Much!

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