I don't understand how to solve. 1. For the exothermic reaction below, increasing the pressure would

N2(g)+3H2(g)⇄2NH3(g)
a. increase [H2]
b. increase [NH3]
c. increase [N2]
d. have no effect

2. If K=100, then the value of K for the reverse reaction is
a. the same value
b. can only be determined by experimentation
c. the negative of the value for the forward reaction
d. 0.01

1. b. increase [NH3].

2. d. 0.01.

Explanation:

Hello!

In this case, for these equilibrium problems, we proceed as follows:

1. Here, we consider the Le C hatelier 's principle applied to a gas-phase reaction in which the reactants side have more number of moles; therefore, increasing the pressure will increase the products side as it has the fewest number of moles, so the answer is b. increase [NH3].

2. Here, we know that the equilibrium constant of the reverse reaction equals the inverse of the equilibrium constant of the forward reaction, thus, we obtain:

Therefore, the answer is d. 0.01.

Best regards!

if you mean hydrogen and oxygen then water is the product

answer: i have one answer

acids are substances that ionize (break off) in an aqueous solution to produce hydrogen (h+) ions

explanation:

hope this and sorry i could only come up with one answer!