Consider the following reaction: CH 4 +2O 2 -> CO 2 + 2H 2 O Consider the follow

Question

Consider the following reaction: CH4 +2O2 -> CO2 + 2H2O

Consider the following reaction CH4 (g) + 202 (g) CO2 (g) + 2H20 (g) a) Is heat absorbed or evolved in the course of this reaction? H," =-890 kJ b) Calculate the amount of heat transferred when 45.0 g of CH4 () is decomposed by this c) For a given sample of CH4 () the enthalpy change on reaction is 66.8 kJ. How many d) What is the value of AH, for the reverse of the previous readtion? How many kioijoules of reaction at constant pressure. grams of H2)areproduced? heat are released when 27.0 g of H2O )reacts completely with CO2g) to form CH4() and 02 () at constant pressure?

Explanation / Answer

(a)

Since deltaH0f is given negative value, heat is released in this reaction

(b)

From the balanced equation 16.0 g. ( 1 mol) of Methane gives - 890 kJ of heat

then,

45.0 g. of methane gives 45.0 * ( - 890 ) / 16.0 = 2503. kJ

(c)

From the balanced equation,

890 kJ of heat is released from 16.0 g. of methane

then, 66.8 kJ of heat is released from 66.8 * 16.0 / 890 = 1.20 g. of methane

(d)

reverse reaction is endothermic reaction. So, deltaHr = + 890 kJ

For the reverse reaction no heat is released but heat is absorbed.

From the balanced equation,

2 * 18.0 g. of water needs 890 kJ of heat.

Then,

27.0 g. of water needs 27.0 * 890 / (36.0) = 667.5 kJ of heat .

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