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how many moles of CO2 form when 58.0 g of butane, C4H10, burn in oxygen? 2C4H10+13O2--->8CO2+10H2O

Sagot :

pyromorphite
2C4H10 + 13O2 ---> 8CO2 + 10H2O 1 mole of C4H10 = 58g According to the reaction: 2*58g of C4H10 ------------- 8 molesof CO2 58g of C4H10 ----------------- x moles of CO2 x = 4 miles od CO2

Answer: 4 moles of [tex]CO_2[/tex] are produced.

Explanation:

To calculate the number of moles, we use the formula:

[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]

For butane:

Given mass of butane = 58g

Molar mass of butane = 58 g/mol

Putting values in above equation, we get:

[tex]\text{Moles of butane}=\frac{58g}{58g/mol}=1mole[/tex]

For the given chemical equation:

[tex]2C_4H_{10}+13O_2\rightarrow 8CO_2+10H_2O[/tex]

By Stoichiometry of the reaction:

2 moles of butane produces 8 moles of carbon dioxide

So, 1 mole of butane will produce = [tex]\frac{8}{2}\times 1=4moles[/tex] of carbon dioxide

Hence, 4 moles of [tex]CO_2[/tex] are produced.

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