Question

Consider the following reaction: 3CH4 + 2H2O + CO2 --> 4CO + 8H2 If the rate...

Consider the following reaction: 3CH4 + 2H2O + CO2 --> 4CO + 8H2 If the rate of disappearance of CO2 is 7.4 M/s, match the remaining compounds with their respective rates of appearance or dissapearance.

CH4, H2O, CO, H2

A.60

B.15

C.22.5

D.30

Homework Answers

Answer #1

Answer: According to the question , here the equation is :

  3CH4 + 2H2O + CO2 --> 4CO + 8H2

Here , -1/3 d[CH4] /dt = -1/2 d[H2O]/dt = -d[CO2]/dt = 1/4 d[CO]/dt = 1/8 d[H2]/dt

And we have , -d[CO2]/dt = 7.4 m/s

so , - d[CH4]/dt = 7.4 * 3 = 22.5 [ Means option [C] ]

for , -d[H2O]/dt = 7.4 * 2 = 14.8 means approx 15 [ hence option [B]

for , d[CO]/dt = 7.4 *4 = 29.6 means approx 30 , hence option [D] .

Now, for , d[H2]/dt = 7.4 * 8 = 59.2 means approx 60 hence option [A] .

So it is all about the given question . Thank you :)

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Consider the following system at equilibrium CH4(g) + 2H2O(g) ↔ CO2(g) + 4H2(g). Suppose the concentration...
Consider the following system at equilibrium CH4(g) + 2H2O(g) ↔ CO2(g) + 4H2(g). Suppose the concentration of H2O is increased. (a) In which direction does the reaction shift to reestablish equilibrium? (b) What happens to the concentrations of CH4, CO2, and H2 as the reaction shifts to reestablish equilibrium?
Consider the following chemical reaction: CH4 + 2O2 → CO2 + 2H2O 4 moles of methane...
Consider the following chemical reaction: CH4 + 2O2 → CO2 + 2H2O 4 moles of methane (CH4) are combined with 5 moles of oxygen (O2). How much carbon dioxide (CO2) will form?
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.120 M...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.120 M COand 0.120 M H2O. A)What will be the equilibrium concentration of [CO]? B)What will be the equilibrium concentration of [H2O]? C)What will be the equilibrium concentration of [CO2]? D)What will be the equilibrium concentration of [H2]?
The reaction between carbon monoxide and water is given below: CO(g) + H2O(l) --------> CO2(g) +...
The reaction between carbon monoxide and water is given below: CO(g) + H2O(l) --------> CO2(g) + H2(g) We therefore know that which of the following reactions can also occur? a)  PbCl2(s) ---------->   Pb(s) + Cl2(g) b) CH4(g) + H2O(g) ----------> CO(g) + 3 H2(g) c) CO(g) + 3 H2(g) ------------------> CH4(g) + H2O(g) d) None of the Above
Consider the following reaction. CO (g) +H2O (g) = CO2 (g) + H2 (g) If the...
Consider the following reaction. CO (g) +H2O (g) = CO2 (g) + H2 (g) If the reaction begins in a 10.00 L vessel with 2.5 mol CO and 2.5 mol H2O gas at 588K (Kc= 31.4 at 588 K). Calculate the concentration of CO, H2O, CO2, and H2 at equilibrium.
Consider the water-gas shift reaction: H2(g) + CO2(g) = H2O(g) + CO(g) A) Find Kp for...
Consider the water-gas shift reaction: H2(g) + CO2(g) = H2O(g) + CO(g) A) Find Kp for this reaction at 298 K B) What is 1) Consider the water-gas shift reaction: H2(g) + CO2(g) = H2O(g) + CO(g). A) Find Kp for this reaction at 298 K. B) What is ΔH° for this reaction? C) What type of pressure and temperature change would favor CO production? D) What is K at 1000 K?
From the following data calculate the ΔHrxn for the following reaction: 2 C(s) + 2 H2O(g)...
From the following data calculate the ΔHrxn for the following reaction: 2 C(s) + 2 H2O(g)  CH4(g) + CO2(g) ΔHrxn = ________ Use the following reactions and given ΔH’s and show your work. CO(g) + H2(g) → C(s) + H2O(g) ΔHrxn = −131.3 kJ CO(g) + H2O(g) → CO2(g) + H2(g) ΔHrxn = −41.2 kJ CO(g) + 3 H2(g) → CH4(g) + H2O(g) ΔHrxn = −206.1 kJ
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 1344 torr and a H2O partial pressure of 1780 torr at 2000 K. calculate the equilibrium partial pressure of CO2. calculate the same for H2.
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 1326 torr and a H2O partial pressure of 1770 torr at 2000 K. A) Calculate the equilibrium partial pressure of CO2. B) Calculate the equilibrium partial pressure of H2.
Consider the following reaction: 2NO(g)+2H2(g)→N2(g)+2H2O(g). If the rate constant for this reaction at 1000 K is...
Consider the following reaction: 2NO(g)+2H2(g)→N2(g)+2H2O(g). If the rate constant for this reaction at 1000 K is 6.0×104M−2s−1, what is the reaction rate when [NO]= 2.90×10−2M and [H2]= 1.80×10−2M? Express your answer using two significant figures. rate =   M/s   SubmitMy AnswersGive Up Part C What is the reaction rate at 1000 K when the concentration of NO is increased to 0.14 M, while the concentration of H2 is 1.80×10−2M? Express your answer using two significant figures.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT