Use Hesss Law and the given combustion equations to determine the enthalpy of reaction for the conversion of butane, C₄H₁₀, into butanol, C₄H₉OH:

C₄H_{10 (g)} + O_{2 (g)} C₄H₉OH _{(l)_} H = ?

Given:

C₄H_{10 (g)} + O_{2 (g)} 4 CO_{2 (g)} + 5 H₂O _(l) H = -2881.9 kJ/mol

C₄H₉OH _(l) + 6 O_{2 (g)} 4 CO_{2 (g)} + 5 H₂O _(l) H = - 2712.9 kJ/mol

Question 9 options:

	169.0 kJ/mol
	5594.8 kJ/mol
	5594.8 kJ/mol
	169.0 kJ/mol

Question 10 (1 point)

Which statement about the rate of a reaction is false?

Question 10 options:

	Assuming temperature is constant, the instantaneous rate of reaction increases over time.
	The instantaneous rate is the slope of the tangent to the curve on a concentration-time graph.
	The higher the rate, the greater is the slope of a line on a concentration-time graph.
	Rates of reaction can be determined from changes in colour, conductivity or volume of gas produced.

Question 11 (1 point)

In the reaction, N_{2 (g)} + O_{2 (g)} --> 2 NO_{2 (g)} , if the concentration of nitrogen dioxide changes from 0.45 mol/L to 1.00 mol/L in 2 minutes, what is the average rate of production of nitrogen dioxide in the system?

Question 11 options:

	3.64 mol/(Lmin)
	0.333 mol/(Lmin)
	12.6 mol/(Lmin)
	0.137 mol/(Lmin)
	0.275 mol/(Lmin)