CH₄(g) + 2O₂(g) = CO₂(g) + 2 H₂O(l) ΔH = -891 kJ

Calculate the enthalpy change for each of the following cases.

(a) 3.00 g methane is burned in excess oxygen.

(b) 1.00 x 10^3 L methane gas at 735 torr and 23°C is burned in excess oxygen. 

SiH₄(g) + 2 F₂(g)= SiF₄(g) + 4 HF(g)

If 19.1 kJ are released when 2.00 g of F2 reacts with an excess of SiH4, what is the heat of the reaction when 1.30 moles of F2 react?

If 19.3 kJ are released when 1.30 g of F2 reacts with an excess of SiH4, complete the thermochemical equation below.

SiH₄(g) + 2 F₂(g) = SiF₄(g) + 4 HF(g)