Calculate the change in energy when 665.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K

So i used the formula
change in energy = change in H - nRT

90.7-51.9-38.8

its wrong i need help

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To calculate the change in energy for a chemical reaction, you can use the formula:

ΔE = ΔH - (n * R * T)

where:
ΔE is the change in energy
ΔH is the change in enthalpy
n is the number of moles of the substance involved in the reaction
R is the ideal gas constant
T is the temperature in Kelvin

In this case, to determine the change in energy when 665.0 g of CH3OH(g) completely reacts, we need to convert the mass of CH3OH(g) into moles. We can use the molar mass to find the number of moles:

Molar mass of CH3OH(g) = (1 * 12.01 g/mol) + (4 * 1.01 g/mol) + (1 * 16.00 g/mol) = 32.04 g/mol

Number of moles = mass / molar mass
Number of moles = 665.0 g / 32.04 g/mol = 20.72 mol (rounded to two decimal places)

Now that we have the number of moles (n = 20.72 mol), we can proceed with the calculation:

ΔE = ΔH - (n * R * T)

Given that R = 8.314 J/mol·K and T = 300 K, and assuming ΔH = 90.7 kJ (which seems to be the missing value in your equation), we can plug in the values:

ΔE = (90.7 kJ) - (20.72 mol * 8.314 J/mol·K * 300 K)

Make sure to convert kJ to J, kJ = 1000 J≈ 90700 J:

ΔE = (90700 J) - (20.72 mol * 8.314 J/mol·K * 300 K)

Calculate the multiplication part:

ΔE = (90700 J) - (49285 J)

Lastly, subtract:

ΔE ≈ 41415 J or 41.4 kJ

So, the change in energy when 665.0 g of CH3OH(g) completely reacts is approximately 41.4 kJ.