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In the equilibrium system below, which of the following changes would cause the equilibrium position to shift to the right? CO(g) + 3H2 (g)CH4 (g) + H2O (g) H = -206 kJ/mol

Chemistry
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I don't see any equilibrium changes listed, and nor is this a reaction since there is no arrow, but assuming that CO(g) and H2 (g) go to CH4(g) and H2O(g) then changes that would shift the eq position to the right would include adding more of the reactants (CO and H2), removing the products (CH4, H20), or, since all components are gases, increasing the pressure, since the system would tend to move from more moles of gas to less. Also, since we know ∆H is negative, the reaction is exothermic, so we can consider this a product, so I *think* having the reaction occur in a vessel that can disperse the accumulated heat will also help.
I see no right side
Here is the Equilibrium: CO(g)+3H2(g)-->/<-- CH4(g)+H2O(g) (triangle) H = -206 kJ/mol (the --->/<-- means the arrows are above each other)

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