HELP
posted by Chemistry .
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
90.751.938.8
its wrong i need help

Indicate your subject in the "School Subject" box, so those with expertise in the area will respond to the question.
Respond to this Question
Similar Questions

cHEMISTRY
Strontium metal is responsible for the red color in fireworks. Fireworks manufacturers use strontium carbonate, which can be produced by combining strontium metal, graphite (C), and oxygen gas. The formation of one mole of SrCO3 releases … 
Chem
I don't believe I'm getting the correct answers for this problem. Could someone look over my work and verify whether it is correct or not? 
Chem
Consider the reaction H2S(g) <==> H2(g) + 1/2S2(g) At 1065*C the partial pressure at equilibrium of hydrogen sulfied, hydrogen and sulfur are found to be .670 atm, .221 atm, and .110 atm, respectively. Find Kp and deltaG* for … 
Chemsitry II
The partial pressure of CH4(g) is 0.185 atm and that of O2(g) is 0.300 atm in a mixture of the two gases. a) What is the mole fraction of each gas in the mixture? 
Chemistry
Calculate the partial pressures and total pressure (in atm) exerted by 0.838 mol of methane, 0.184 mol of ethane and 0.755 mol of neon contained in a 4.00 L container at 27 C. PV=nRT for methane (4.00L) X = (0.838 mol)(0.08206 Latm/molK)(300.15 … 
chemistrycheck answer
I was wondering if someone can tell me if I did this right: The gas constant (R) has many different unit formulations. Convert the value of 8.314 (m3Pa)/(Kmol) into units of (LmmHg)/(Kmol). This is what I did: (8.314 m3Pa/Kmol)*(1 … 
chemistryrecheck answer
I was wondering if someone can tell me if I did this right: The gas constant (R) has many different unit formulations. Convert the value of 8.314 (m3Pa)/(Kmol) into units of (LmmHg)/(Kmol). This is what I did: (8.314 m3Pa/Kmol)*(1 … 
chemistry
A 79.9L sample of a gaseous hydrocarbon, measured at 1.00 atm pressure and 25.0°C, is burned in excess oxygen, liberating 4.24 × 10^3 kJ of heat at constant pressure. What is the identity of the hydrocarbon? 
chemistry
the pressure of 3moles of an ideal gas in a container is reduced from 1.0 atm to 0.50 atm against a constant pressure of 0.50 atm at a constant temperature of 273K..what is the change of heat (in J) for the process? 
Chemisty
Calculate the Volume occupied by 1.5 moles of an ideal gas at 25 degrees Celsius and a pressure of 0.80 atm. (R= 0.08206 L atm/(mol*K). I've tried using the ideal gas law: PV=nRT but i can't seem to get where I am getting lost. V=(1.5mol)(0.08206 …