# Problem: In which reaction does Kp = Kc? a) NO(g) + O2(g) &lt;--&gt; N2O3(g) b) N2(g) + O2(g) &lt;--&gt; 2NO(g) c) CaCO3(s) &lt;--&gt; CaO(s) + CO2(g) d) N2(g) + H2O(g) &lt;--&gt; NO(g) + H2(g) e) None

###### FREE Expert Solution

We are asked to choose among the given reactions for which Kp = Kc.

The concentration equilibrium constant Kc is related to the pressure equilibrium constant Kp by the equation:

$\overline{){{\mathbf{K}}}_{{\mathbf{p}}}{\mathbf{=}}{{\mathbf{K}}}_{{\mathbf{c}}}{\left(\mathbf{R}\mathbf{T}\right)}^{\mathbf{∆}\mathbf{n}}}$

Where:

R = ideal gas constant (0.08206 L∙atm/mol∙K)

T = temperature in Kelvin

∆n = change in gaseous moles

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###### Problem Details

In which reaction does Kp = Kc

a) NO(g) + O2(g) <--> N2O3(g)

b) N2(g) + O2(g) <--> 2NO(g)

c) CaCO3(s) <--> CaO(s) + CO2(g)

d) N2(g) + H2O(g) <--> NO(g) + H2(g)

e) None

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Chemical Equilibrium concept. You can view video lessons to learn Chemical Equilibrium. Or if you need more Chemical Equilibrium practice, you can also practice Chemical Equilibrium practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Mines' class at OAKTON.