What volume of butane can be produced from the reaction of 13.45 g of carbon and 17.65 l of hydrogen gas

Complete Question

What volume of butane can be produced from the reaction of 13.45 g of carbon and 17.65 L of hydrogen gas at STP ?

The volume of butane produced is

Explanation:

From the question we are told that

     The mass of carbon is  

    The volume of hydrogen is

The number of moles of carbon is mathematically evaluated as

Where is the molar mass of carbon which is a constant with value

So  

Now since the volume of the  hydrogen is measured at standard temperature and pressure

    Hence the number of moles of hydrogen is  

Where 22.4 is a constant

Comparing we see that hydrogen is the limiting reactant

because is  greater than

The chemical equation for this reaction is

looking at chemical equation we see that

   5 moles of hydrogen gas reacts with 4 moles of  carbon to produce 1 mole of  butane

 This implies that

   0.79 moles react with 1.12 moles of carbon to produce x moles of butane

Therefore

Now since this reaction is carried out at standard temperature and pressure the volume of butane produced will be

8 m/s because for him to get the same amount of energy as ray is putting out, bobby, who weighs half as much as ray, needs to run twice as fast.