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Consider the reaction at 300 Kelvin H2 CL2=to HCL gas calculate delta u if 3 mole of H2 completely react with any mole of cl2 to form HCL?
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Consider the reaction at 300 Kelvin H2 CL2=to HCL gas calculate delt...
Reaction:
The reaction given is:
H2 + Cl2 → 2HCl

Stoichiometry:
According to the balanced equation, 1 mole of Cl2 reacts with 1 mole of H2 to produce 2 moles of HCl.

Given Information:
Temperature (T) = 300 K
Number of moles of H2 (n) = 3 moles

Calculation of ΔU:
The change in internal energy (ΔU) can be calculated using the equation:
ΔU = ΔH - ΔnRT

Step 1: Calculate ΔH:
The enthalpy change (ΔH) can be determined using the bond enthalpy values of the reactants and products.

Bond Enthalpy Values:
H–H = 436 kJ/mol
Cl–Cl = 242 kJ/mol
H–Cl = 431 kJ/mol

Calculating ΔH:
ΔH = (Σ Bond energies of reactants) - (Σ Bond energies of products)
= (1 * H–H) + (1 * Cl–Cl) - (2 * H–Cl)
= (1 * 436) + (1 * 242) - (2 * 431)
= 678 kJ/mol

Step 2: Calculate Δn:
Δn = (moles of gaseous products) - (moles of gaseous reactants)
= (2 * 3) - (1 * 3)
= 3 moles

Step 3: Calculate ΔU:
The ideal gas constant (R) is 8.314 J/(mol·K).

ΔU = ΔH - ΔnRT
= 678 kJ/mol - (3 mol * 8.314 J/(mol·K) * 300 K)
= 678 kJ/mol - 7478.2 J
= 678 kJ/mol - 7.4782 kJ
= 670.5218 kJ/mol

Final Answer:
The change in internal energy (ΔU) for the reaction of 3 moles of H2 with any mole of Cl2 to form HCl gas at 300 K is approximately 670.5218 kJ/mol.
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Consider the reaction at 300 Kelvin H2 CL2=to HCL gas calculate delta u if 3 mole of H2 completely react with any mole of cl2 to form HCL?
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