For the reaction, C(s)+CO2(g) arrow 2CO(g), Kp = 63 atm at 1000 K. If at equilibrium PCO = 10 Pco2, than the total pressure of the gases at equilibrium is

Question

For the reaction, C(s)+CO2(g) arrow 2CO(g), Kp = 63 atm at 1000 K. If at equilibrium PCO = 10 Pco2, than the total pressure of the gases at equilibrium is (A) 6.3 atm (B) 6.93 atm (C) 0.63 atm (D) 0.693 atm

Tardigrade Admin · Accepted Answer

Kp = (p2CO/PCO2) 63 = l00x or x = 0.63 Total equilibrium pressure = 6.3 + 0.63 = 6.93 atm

Q. For the reaction, $C_{(s)} + C O_{2 (g)} \to 2 C O_{(g)},$ $K_{p} = 63$ atm at $1000 K$ . If at equilibrium $P_{CO} = 10 P c o_{2},$ than the total pressure of the gases at equilibrium is

6.3 atm

6.93 atm

0.63 atm

0.693 atm

69.3 atm

$K_{p} = \frac{p _{CO}^{2}}{P _{C O_{2}}}$ 63 = l00x or x = 0.63
Total equilibrium pressure = 6.3 + 0.63 = 6.93 atm

Q. For the reaction, C(s)​+CO2(g)​→2CO(g)​, Kp​=63 atm at 1000K. If at equilibrium PCO​=10Pco2​, than the total pressure of the gases at equilibrium is