Let us assume that the solution is 100g in total.

Given, mass of CO = 90.55 g

Now, the mass of CO_{2} = (100 – 90.55) = 9.45 g

Now, number of moles of CO,

\( n_{CO}=\dfrac{90.5}{28}=3.234\: mol\)

Number of moles of CO_{2},

\( n_{CO_{2}}=\dfrac{9.45}{44}=0.215\: mol\)

Partial pressure of CO,

\( PCO= \dfrac{n_{CO}}{n_{CO}+n_{CO_{2}}}\times p_{total} \)

\( =\dfrac{3.234}{3.234+0.215}\times 1=0.938\)

Partial pressure of CO_{2},

\( P_{CO_{2}}=\dfrac{n_{CO_{2}}}{n_{CO}+n_{CO_{2}}}\times p_{total}\)

\( =\dfrac{0.215}{3.234+0.215}\times 1=0.062, atm\)

Therefore,

\( Kp= \dfrac{[CO]^{2}}{[CO_{2}]}\\ \\ \)

\( =\dfrac{(0.938)^{2}}{0.062}\\ \\ \)

\(=14.19\)

For the given reaction,

∆n = 2 – 1 = 1

We know that,

\(Kp = Kc(RT) ^{\Delta n}\)

\( \Rightarrow 14.19 = K_{c}(0.082\times 1127)^{1}\\ \\ \Rightarrow K_{c}\)

\( =\dfrac{14.19}{0.082\times 1127}\\ \\ \)

\( =0.154(approximately)\)

Answered by Pragya Singh | 1 year agoThe concentration of sulphide ion in 0.1M HCl solution saturated with hydrogen sulphide is 1.0 × 10^{–19} M. If 10 mL of this is added to 5 mL of 0.04M solution of the following: FeSO_{4}, MnCl_{2}, ZnCl_{2} and CdCl_{2} . in which of these solutions precipitation will take place?

What is the minimum volume of water required to dissolve 1g of calcium sulphate at 298 K? (For calcium sulphate, K_{sp} is 9.1 × 10^{–6}).

What is the maximum concentration of equimolar solutions of ferrous sulphate and sodium sulphide so that when mixed in equal volumes, there is no precipitation of iron sulphide? (For iron sulphide, Ksp = 6.3 × 10^{–18}).

The ionization constant of benzoic acid is 6.46 × 10^{–5} and Ksp for silver benzoate is 2.5 × 10^{–13}. How many times is silver benzoate more soluble in a buffer of pH 3.19 compared to its solubility in pure water?

Equal volumes of 0.002 M solutions of sodium iodate and cupric chlorate are mixed together. Will it lead to precipitation of copper iodate? (For cupric iodate K_{sp} = 7.4 × 10^{–8} ).