Combining chemical equations

[IreneGi2I]

For Sapling #5, I got the answer by multiplying equilibrium constants for two relevant chemical equations.

Do we always multiply equilibrium constants when combining chemical equations? Or, would there be other ways to solve problems like this?

[Ryan Hoang 1D]

If we're adding two equations together, we would multiply the equilibrium constants. If we're subtracting, then we'd divide.

[Hannah Alltucker 3L]

I don't know if there is a more efficient way, but as long as we all remember to use the radical when the reaction is reversed, and know to make whatever our multiplying coefficient for a reaction equation is our power for that K, we should be fine. think this method itself is probably straightforwards enough, but we'll have to see what else he teaches us.

[SophiaBarden 2E]

There are a couple rules when dealing with equilibrium constants and combining equations. When you are adding two equations together, then you multiple the Ks together. When youre substracting one reaction from another, then you divide respectively. But remember when youre manipulating on equation to match another, then multiplying an equation would mean cubing the K to that number. Also reversing a reaction, you must multiply K to the power of -1.

[Irene Chang 2F]

In addition to multiplying the constants when you add them together, you also have to look out for if you are multiplying the entire equation by a constant. For example, if you were to change H2 + I2 <--> 2HI into 2H2 + 2I2 <--> 4HI, you would need to square the K value.

[Margaret Wang 2D]

When combining different reactions, multiplication is used for adding reactions and division is used for subtracting reactions. Adding and subtracting the equilibrium constant values never happens.