The equilibrium constant for the reaction `CO(g)+H_(2)O(g)hArrCO_(2)(g)+H_(2)(g) is 5` how many moles of `CO_(2)` must be added to 1 litre container alrady containing 3 moles each of CO and `H_(2)O` to make 2 M equilibrium conentration of CO?
For the reactions : C(s) + O_(2) (g) to CO_(2) (g)
Write the equilibrium constant expression for the following reactions. CH_(4)(g) + 2O_(2)(g) hArr CO_(2)(g) + 2H_(2)O(l)
At a certain temperature the equilibrium constant K_(c) is 0.25 for the reaction A_(2)(g)+B_(2)(g)hArrC_(2)(g)+D_(2)(g) If we take 1 mole of each of the four gases in a 10 litre container ,what would be equilibrium concentration of A_(2) (g)?
The equilibrium constant K_(p) for the reaction H_(2)(g)+CO_(2)(g)hArrH_(2)(g)+CO(g) is 4.0 at 1660^(@)C Inittally 0.80 H_(2) and 0.80 mole CO_(2) are injecteed into a 5.0 litre flask what is the equilibrium concentraton of CO_(2)(g) ?
Consider the reaction 2CO(g)+O_(2)(g)hArr2CO_(2)(g)+Heat Under what conditions shift is undetminable ?
The equilibrium constant K_(c) for the reaction SO_(2) (g) + NO_(2)(g)hArrSO_(3)(g)+NO(g) is 16 . 1 mole of each of all the four gases is taken in 1dm^(3) vessel , the equilibrium concentration of NO would be:
Balance the following equation : CH_4(g) +O_2(g) rarr CO_2 (g)+H_2O(l)
What is the mass of 0.1 mole of CO_2 in g ?
For the reaction XCO_(3)hArrXO(s)+CO_(2)(g), K_(p)=1.642 atm" "at727^(@)C " If 4 moles of" XCo_(3)(s) was put into a 50 litre container and heated to 727^(@)C What mole percent of the XCO_(3) remains unreacted at equilibrium ?
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
