For chemical reactions involving ideal gases, the equilibrium constant K can be expressed either in terms of the concentrations of the gases (in M) or as a function of the partial pressures of the gases (in atmospheres). In the latter case, the equilibrium constant is denoted as Kp to distinguish it from the concentration-based equilibrium constant K. PART A:

For the reaction

2CH4(g)?C2H2(g)+3H2(g)

K = 0.150 at 1696?C . What is Kp for the reaction at this temperature?

Express your answer numerically.

PART B:

For the reaction

N2(g)+3H2(g)?2NH3(g)

Kp = 2.55

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation:

i'm pretty sure it is letter c.) car

c. electrical charges of ionic bonds.