Consider the following intermediate chemical equations. AH, = 74.6 kJ CH2(g)-> C(s)+ 2H2(g) CCl2(g) - C(s) + 2C1,(g) H2(g)+Cl,(g) → 2HCl(g) AH, = 95.7 kJ AH, --92.3kJ What is the enthalpy of the overall chemical reaction CH (9)+401,(g) → CCI(g) +4HCl(g)? -205.7 kJ -113.4 kJ O-14.3 kJ O 78.0 kJ​

according to kinetic-molecular theory, the following would not be considered an ideal gas:

a gas at very low volumes, when gas particles are very close together

a gas at very low temperatures, when gas particles have very little kinetic energy a gas

a gas with highly polar molecules that have very strong intermolecular forces

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as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2