Question

In: Chemistry

Consider the water-shift gas reaction: H2O + CO --> H2 + CO2 A closed reaction vessel...

Consider the water-shift gas reaction:

H2O + CO --> H2 + CO2

A closed reaction vessel maintained at 3000 degrees Celcius is filled with 0.475 M H2 and 0.490 M CO2. At equilibrium, their respective concentrations are 0.410 and 0.425 M.

PART A:

The following ratio represents

[H2][CO2] / [H2O][CO]

CHOOSE ONE OR MORE:

the law of mass action, the mass action expression, the equilibrium constant expression, the equilibrium constant. none of these

PART B:

which way must the system shift in order to attain equilibrium

CHOOSE ONE

to the right, to the left, cannot be determined

PART C:

the value 41.0, represents

CHOOSE ONE OR MORE

the law of mass action, the mass action expression, the equilibrium constant expression, the equlibrium constant, none of these

PART D:

The equilibrium constant, Kc, is unitless, why?

CHOOSE ONE

in the expression for Kc, molarities are always used so units are redundant

the cncentrations in K are theoretically ratios of the concentrations to an ideal standard 1.000 M

the concentration units are ignored. K actually has units if there aren't equal numbers of M units in thenumerator and the denominator

Solutions

Expert Solution

queen_honey_blossom answered 2 years ago
Next > < Previous

Related Solutions

The water-gas shift reaction (CO + H­2O à CO2 + H­2) occurs in a series of...
The water-gas shift reaction (CO + H­2O à CO2 + H­2) occurs in a series of two reactors. An equimolar mixture of steam and CO (stream 1) enters the first reactor. The product stream from the first reactor (stream 3) and an additional stream (stream 3) containing pure steam enter the second reactor. The fractional conversion of CO in the first reactor is 0.610, and the fractional conversion of CO in the second reactor is 0.790. The product stream has...
The water-gas shift reaction (CO + H­2O à CO2 + H­2) occurs in a series of...
The water-gas shift reaction (CO + H­2O à CO2 + H­2) occurs in a series of two reactors. An equimolar mixture of steam and CO (stream 1) enters the first reactor. The product stream from the first reactor (stream 3) and an additional stream (stream 3) containing pure steam enter the second reactor. The fractional conversion of CO in the first reactor is 0.610, and the fractional conversion of CO in the second reactor is 0.790. The product stream has...
Consider the following reaction: CO (g) + H2O (g) ⇌ CO2 (g) + H2(g) If you...
Consider the following reaction: CO (g) + H2O (g) ⇌ CO2 (g) + H2(g) If you start with a mixture containing 1.00 mol of CO and 1.00 mol of H2O, calculate the number of moles of each component in the mixture when equilibrium is reached at 1000 °C. The mixture contains 0.43 mol H2? nCO = nH2O = nCO2 = How do I work this out?
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1336 torr and a H2O partial pressure of 1764 torr at 2000 K. Part A Calculate the equilibrium partial pressure of CO2. Part B Calculate the equilibrium partial pressure of H2.
Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) K=0.118 at 4000 K A reaction mixture initially contains a CO partial...
Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) K=0.118 at 4000 K A reaction mixture initially contains a CO partial pressure of 1361 mbar and a H2O partial pressure of 1781 mbar at 4000 K. Part A: Calculate the equilibrium partial pressure of CO in bar using three decimal places Part B: Calculate the equilibrium partial pressure of H2O in bar using three decimal places. Part C: Calculate the equilibrium partial pressure of CO2 in bar using three decimal places Part D: Calculate the...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1390 torr and a H2O partial pressure of 1710 torr at 2000 K. Calculate the equilibrium partial pressure of CO2.
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1390 torr and a H2O partial pressure of 1770 torr at 2000 K. A) Calculate the equilibrium partial pressure of CO2.
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1346 torr and a H2O partial pressure of 1762 torr at 2000 K. A.) Calculate the equilibrium partial pressure of CO2. B.) Calculate the equilibrium partial pressure of H2
Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.135 M CO...
Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.135 M CO and 0.135 M H2O. What is the equilibrium concentration of [CO], [H2O], [CO2], and [H2]
16.60 Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a...
16.60 Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1332 torr and a H2O partial pressure of 1772 torr at 2000 K . Part A: Calculate the equilibrium partial pressure of CO2 . Part B: Calculate the equilibrium partial pressure of H2 .
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT