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Consider the following reaction.
CH3OH(g) -> CO(g) + 2 H2(g) H = +90.7 kJ

Calculate delta E when 845.0 g of CH3OH(g) completely reacts at aconstant 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

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Reid Wolff
Reid WolffLv2
28 Sep 2019

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Related questions


14. Consider the following reaction:
2AgCl(s)  2Ag(s) + Cl2(g) H° = 127.1 kJ; S° = 115.7 J/K at 298 K
Suppose 41.0 g of silver(I) chloride is placed in a 70.0 L vessel at 298 K. When
equilibrium is reached, what will the partial pressure of chlorine gas be?
(R = 0.0821 L · atm/(K · mol) = 8.31 J/(K · mol))
A) 0.050 atm B) 5.1  10–23 atm C) 0.95 atm
D) 0.10 atm E) 5.7  10–17 atm

1)For a given reaction, the rate constant doubles when the temperature is increased from 43.5 °C to 71.5 °C. What is the activation energy for this reaction? (R = 8.314 J/K×mol)
___kJ/mol

2)The vapor pressure of liquid carbon tetrachloride, CCl4, is 100. mm Hg at 296 K. A 0.173 g sample of liquid CCl4 is placed in a closed, evacuated 370. mL container at a temperature of 296 K. The molecular mass of carbon tetrachloride equals 153.82 g/mol. (R = 0.08206 L*atm/mol*K, and 1 atm = 760 mmHg)
What will the pressure in the container be when equilibrium is reached?____mm Hg

3)

For the second-order reaction below, the initial concentration of reactant A is 0.227 M. If the rate constant for the reaction is 1.03E-2 M–1s–1, what is the concentration of A after 244 seconds?

2A → B + C rate = k[A]2

_____ M

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