General Chemistry Answers

One hundred kilomoles of wet natural gas containing a mixture of methane (CH4) and ethane (C2H6) are combusted. The mole ratio of total carbon to total hydrogen in fuel is given as 13:50. Assuming complete combustion and 50% excess air entering the combustion chamber, compute for the following:

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This coal gas can be used a fuel: CO(g) + H2(g) + O2(g) → CO2(g) + H2O(g) ∆Ho= ?

One hundred kilomoles of wet natural gas containing a mixture of methane (CH4) and ethane (C2H6) are combusted. The mole ratio of total carbon to total hydrogen in fuel is given as 13:50. Assuming complete combustion and 50% excess air entering the combustion chamber, compute for the following:

How much air in kmoles is entering the combustion chamber?

Percent of ethane in the fuel is?

How much water was formed? 

Theoretical oxygen needed in kmoles is

Amount in kmoles of carbon dioxide found in the flue gas is

Percent of methane in the fuel is

Total number of kmoles in the flue gas is

What is the theoretical air needed in kmoles? 

Write the balanced overall equation for the followingprocess (equation 3) and calculate

∆HoveralI.

(1) N2 (g) + O2(g) → 2NO(g) ∆H = 180.6 kJ

(2) 2NO(g) + O2(g) → 2NO2(g) ∆H = - 114.2 kJ

(3) ∆Hoverall=?

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If you had excess aluminum, how many moles of aluminum chloride could be produced from 18.0g of chlorine gas, Cl_2?

How many molecules of NH₃ are produced from 2.33x10^-4 of H₂

Atoms of element H (Chlorine) combined to form diatomic molecules at room temperature. Explain the melting point and boiling point of molecule H.

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