Question

Consider the following reaction: CH$_4$(g) + 2O$_2$(g) $\rightarrow$ CO$_2$(g) + 2H$_2$O(l) $\Delta$H = -891 kJ a. Calculate the enthalpy change if 5.42 g methane is burned in excess oxygen. Enthalpy change = 301.8 kJ b. Calculate the enthalpy change if 6.22 $\times$ 10$^3$ L methane gas at 732 torr and 25$^\circ$C is burned in excess oxygen. Enthalpy change = 218442 kJ

          Consider the following reaction:
CH$_4$(g) + 2O$_2$(g) $\rightarrow$ CO$_2$(g) + 2H$_2$O(l)
$\Delta$H = -891 kJ
a. Calculate the enthalpy change if 5.42 g methane is burned in
excess oxygen.
Enthalpy change = 301.8 kJ
b. Calculate the enthalpy change if 6.22 $\times$ 10$^3$ L methane gas at
732 torr and 25$^\circ$C is burned in excess oxygen.
Enthalpy change = 218442 kJ

Consider the following reaction:
CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)
ΔH = -891 kJ
a. Calculate the enthalpy change if 5.42 g methane is burned in
excess oxygen.
Enthalpy change = 301.8 kJ
b. Calculate the enthalpy change if 6.22 × 10^3 L methane gas at
732 torr and 25^∘C is burned in excess oxygen.
Enthalpy change = 218442 kJ

Added by Eduardo M.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Luke Monroe

Step 1

We can use the following formula: Enthalpy change = (H/mol) x n where H is the enthalpy change given in kJ, mol is the molar mass of methane (16.04 g/mol), and n is the number of moles of methane burned. First, we need to calculate the number of moles of Show more…

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Consider the following reaction: CH4 (g) + 2O2 (g) â†’ CO2 (g) + 2H2O (g) Î”H = -891 kJ a. Calculate the enthalpy change if 5.42 g methane is burned in excess oxygen: Enthalpy change = 301.8 kJ b. Calculate the enthalpy change if 6.22 x 10^3 L methane gas at 732 torr and 25Â°C is burned in excess oxygen: Enthalpy change = 218442 kJ