In the presence of excess oxygen, methane gas burns in a constant ...

[jenna1]

Question 1

When 1.50 mol of CH4(g) reacts with excess Cl2(g) at constant pressure according to the chemical equation shown below, 1062 kJ of heat are released. Calculate the value of ΔH for this reaction, as written.

2CH4(g) + 3Cl2(g) → 2CHCl3(l) + 3H2(g)

Δ rH° = ?

◦ +1420 kJ mol^-1
◦ -708 kJ mol^-1
◦ +708 kJ mol^-1
◦ -1420 kJ mol^-1

Question 2

In the presence of excess oxygen, methane gas burns in a constant pressure system to yield carbon dioxide and water:

CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l)

Δ rH = -890.0 kJ

Calculate the value of q (kJ) in this exothermic reaction when 1.90 g of methane is combusted at constant pressure.
◦ 29.3 kJ mol^-1
◦ -1.06 × 10^-5 kJ mol^-1
◦ 0.0342 kJ mol^-1
◦ -106 kJ mol^-1
◦ -0.00946 kJ mol^-1

[amandanbreshears]

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[jenna1]

Gracias!

[mcabuhat]

Thanks for the timely response, appreciate it