Question

Hydrogen is used as a rocket fuel because itis very light and reacts explosively and completely with oxygen.For the combustion reaction

${\rm 2 H}_{2} (g) + {\rm O}_{2} (g) \rightleftharpoons 2 {\rm H_2O} (g)$

what is the likely magnitude of the equilibrium constant ?

Part B

The industrial production of lime ( $\rm CaO$ ) from calcium carbonate isaccomplished via the following reaction:

${\rm CaCO}_{3} (s) \rightleftharpoons {\rm CaO} (s) + {\rm CO}_{2} (g)$

Given the following data:

Temperature ( $\rm K$ )
298	$1.93\times 10^{-23}$
1200	1.01

what can be said about this reaction?

Lowertemperatures result in more lime formation. The reactionmakes more lime at higher temperatures. The reactiongoes to completion at 1200 $\rm K$ . Theequilibrium lies far to the right at room temperature.

Answer 1

Part A =K>10^3

Answer 2

Part B Chem Reaction produces more lime at high temperatures