Chemistry, 20.07.2019 04:00 evandlubbep6bsvu

What mass of butane in grams is necessary to produce 1.5×103 kj of heat what mass of co2 is produced?

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Answer from: yolo3745

The heat of reaction (i.e. combustion) of butane ( $C_{4} H_{10}$ ) when reacted with oxygen ( $O_{2}$ )  is -2658 kJ/mol butane, and the chemical reaction is given by:

$C_{4} H_{10}$ + $\frac{13}{2} O_{2}$ ---> $4 CO_{2}$ + $5 H_{2}O$

The mass of butane required in the reaction is based on the heat produced by the reaction, which is given to be -1,500 kJ. The minus sign is added because the reaction releases heat (exothermic), which means that the products are in a "lower energy state" than the reactants.

Dividing this with the heat of reaction per mole of butane reacted would give the number of moles butane required. Then, multiplying the answer with the molar mass of butane which is 58 grams/mole, will give the mass of butane required.

Moles of butane = [(-1,500 kJ)/(-2658 kJ/mol butane)]
Moles of butane = 0.5643 moles butane

Mass of butane  = 0.5643 moles butane * 58 grams/mol butane
Mass of butane = 32.73 grams butane

The mass of carbon dioxide ( $CO_{2}$ ) can be determined by multiplying the moles of butane ( $C_{4} H_{10}$ ) with the mole ratio of ( $CO_{2}$ ) produced to the ( $C_{4} H_{10}$ ) reacted, and then with the molar mass of ( $CO_{2}$ ), which is 44 grams/mole.

Mass of carbon dioxide produced
= 0.5643 moles butane * [4 moles $CO_{2}$ / 1 mole $C_{4} H_{10}$ ] * 44 grams/mole $CO_{2}$

Mass of carbon dioxide produced
= 99.32 grams $CO_{2}$

Thus, the mass of butane required is 32.73 grams, and the mass of carbon dioxide produced from the reaction of this amount of butane is 99.32 grams.

Answer from: Kimberley5752

32.73 g of Butane is necessary to produce 1500 kJ of energy and Carbon dioxide produced is 99.32 g.

Molar mass of butane is 58g/mol.

Molar mass of Carbon dioxide is 44g/mol.

In the combustion reaction, 1mol butane produce 2658 kJ of energy.

Moles of butane =

$\rm \bold { \Rightarrow \frac{1,500 }{2658} }\\\rm \bold { \Rightarrow0.564 mol}$

Mass of butane

$\rm \bold {0.5643\times 58 } }\\\rm \bold {32.73 g}$

1 mol of butane produce 4 moles of Carbon dioxide.

Hence,

Mass of Carbon dioxide will be $\rm \bold{ 4\times 32.73g= 99.32 g}$

Hence we can conclude that 32.73 g of Butane is necessary to produce 1500 kJ of energy and Carbon dioxide produced is 99.32 g.

To know more about molar mass, you can refer to the link:

link

Answer from: Quest

answer: $2c_5h_5+1fe\rightarrow 1fe(c_5h_5)_2$

the reaction is type of combination reaction.

explanation:

$? c_5h_5+? fe\rightarrow ? fe(c_5h_5)_2$

on the product side, there are 2 molecules of $c_5h_5$ bonded to fe which means one atom of fe are combined two molecules of $c_5h_5$ . so, balanced chemical equation becomes :

$2c_5h_5+1fe\rightarrow 1fe(c_5h_5)_2$

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.

$a+b\rightarrow ab$

Answer from: Quest

The reaction will shift to the right

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