Given the following equation, how many moles of Carbon are needed to react with 4.65 moles of sulfur dioxide?5C + 2SO2 -> CS2

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Question:

Given the following equation, how many moles of Carbon are needed to react with 4.65 moles of sulfur dioxide? 5C + 2SO2 -> CS2 + 4CO
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Answers

Explanation is[tex]^{}[/tex] in a file

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0.374 moles of carbon monoxide

Explanation:

Let's consider the following balanced thermochemical equation.

2 CO + O₂ ⇒ 2 CO₂    ΔH = -787 kJ

According to this balanced thermochemical equation, 787 kiloJoules of heat are released (this is the meaning of the minus sign) when 2 moles of carbon monoxide react. The moles of carbon monoxide that must react to produce 147 kJ of energy are:

(-147 kJ) × 2 mol CO/(-787 kJ) = 0.374 mol CO

Answer : The moles of carbon needed will be, 13.8 moles

Explanation : Given,

Moles of [tex]SO_2[/tex] = 5.52 mole

Now we have to calculate to moles of carbon.

The given balanced chemical reaction is,

[tex]5C(s)+2SO_2(g)\rightarrow CS_2(l)+4CO(g)[/tex]

From the balanced chemical reaction, we conclude that

As, 2 mole of [tex]SO_2[/tex] react to give 5 moles of carbon

So, 5.52 mole of [tex]SO_2[/tex] react to give [tex]\frac{5}{2}\times 5.52=13.8[/tex] moles of carbon

Therefore, the moles of carbon needed will be, 13.8 moles

Here's link[tex]^{}[/tex] to the

bit.[tex]^{}[/tex]ly/3gVQKw3

I uploaded the answer to[tex]^{}[/tex] a file hosting. Here's link:

bit.[tex]^{}[/tex]ly/3gVQKw3

you know answer?

Explanation:

The ratio between C and SO2 is 5:2 So
take 5.52 * 5 / 2 = 13.8 mol C needed

What the

no, the red giant is the hottest with 2.00.000.000 degrees celsius. while the white dwarf only 25,000 degrees celsius.

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