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) δh = -890.0 kj
calculate the value of q (kj) in this exothermic reaction when 1.70 g of methane is combusted at constant pressure.
(a) -94.6 kj
(b) 0.0306 kj
(c) -0.0106 kj
(d) 32.7 kj
(e) -9.46 × 10^4 kj

The energy released will be -94.56 kJ or -94.6 kJ.

Explanation:

The molar mass of methane is 16g/mol

The given reaction is:

the enthalpy of reaction is given as  ΔH = -890.0 kJ

This means that when one mole of methane undergoes combustion it gives this much of energy.

Now as given that the amount of methane combusted = 1.70g

The energy released will be:

i wish i could but this one is weird give me abc and i can solve it.

answer : (a) volume of the gas = 8.67 ×   l

                (b) second virial coefficient b = -1.21226 l/mole

solution :   given,     t = 300k

                                p = 20atm

                                z = 0.86

                                n = 8.2 mmoles = 8.2 × moles

                                r =   0.082 l atm/k/mol

        find,     (a) volume of gas   and (b) second virial coefficient b at 300k.

formula used :            

                          and            

(a)            

                    = \times 0.082\times 300}{20}[/tex]

                    = 8.67 ×   l

(b)      

                    = (0.00867-1) × 8.659

                    = - 8.5839 l/mole