A 70.0g sample of N2 gas occupies 43.5 L at 45 oC and 1.50 atm of pressure. Some gas is removed from the container. The pressure and temperature now read 1.00 atm and 50oC, respectively. How many moles of gas are in the container now? Assume the volume of the container does not change.

Calculate the standard enthalpy of formation of liquid methanol, ch3oh(l), using the following information: c(graphite) + o2 latex: \longrightarrow ⟶ co2(g) latex: \delta δ h° = –393.5 kj/mol h2(g) + o2 latex: \longrightarrow ⟶ h2o(l) latex: \delta δ h° = –285.8 kj/mol ch3oh(l) + o2(g) latex: \longrightarrow ⟶ co2(g) + 2h2o(l) latex: \delta δ h° = –726.4 kj/mol