Calculate the equilibrium constant for the reaction using the balanced chemical equation and the concentrations of...
Calculate the equilibrium constant for the reaction using the balanced chemical equation and the concentrations of the substances at equilibrium.
Use the
appropriate significant figures in reporting the
answers.
| CO(g) + H2O(g) ⇌ CO2(g) + H2(g) | [CO] = 0.0590 M; [H2O] = 0.00600 M; |
[CO2] = 0.0410 M; [H2] = 0.0410 M |
K =
Homework Answers
![Given- [H2] since the cbove quationis balanced lort, 0.04 to M 亡02 Putting the valite com cautrations 0 eactant and ldletcts](http://img.homeworklib.com/questions/79e8bc60-6444-11eb-83e1-f32b9bd06e25.png?x-oss-process=image/resize,w_560)
Add Answer to:
Calculate the equilibrium constant for the reaction using the
balanced chemical equation and the concentrations of...
Part A Calculate the equilibrium concentrations of CO2, H2, CO, and H.O at 298 Kif the...
Part A Calculate the equilibrium concentrations of CO2, H2, CO, and H.O at 298 Kif the initial concentrations are CO2-0.700 M and [H] -0.400 M The equilibrium constant for the reaction CO2(x) + H2(g) + CO(x) + H2O(R) is 9.71 x 10 at 298 K Express your answers in moles per liter to three significant figures separated by commas VO AE ? (CO, (H). (CO). [H0] M Denne
For the reaction N2(g) + 3H2(g) = 2NH3(g) what is the value of Ke at 500°C if the equilibrium concentrations...
For the reaction N2(g) + 3H2(g) = 2NH3(g) what is the value of Ke at 500°C if the equilibrium concentrations are as follows: [H2] = 0.40 M, (N2) = 0.40 M, and (NH3) = 1.9 M Express the equilibrium constant to two significant figures. V AE OE ? Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining Set up the equilibrium-constant expression for this reaction using the equilibrium concentrations. The product concentrations a the reactant concentrations are...
Calculate Kc for the following reaction given the following equilibrium concentrations of H2(g) = 1.60 M...
Calculate Kc for the following reaction given the following
equilibrium concentrations of
H2(g) = 1.60 M CO(g) = .0030 M, and H2O(g) = 0.030 M. C(s) +
H2O(g) = CO(g) + H2(g)
(Hint: You DO include H2O(g) in the equilibrium expression)
K = ?
Save Answer Calculate K, for the following reaction given the following equilibrium concentrations of H2(9) = 1.60 M COO) = .0030 M, and H,00 = 0.030 M. Co+H,09 = COO + H2(9) (Hint: You Do include H,0...
Solve these two questions plz ASAP 6. Consider the chemical equation and equilibrium constant for the...
Solve these two questions plz
ASAP
6. Consider the chemical equation and equilibrium constant for the synthesis of ammonia at 25 °C: Ng(g) + 3 H2(g-2NH3(g) K=3.7 x 108 Calculate the equilibrium constant for the following reaction at 25 C: 7. Given the equilibrium constants for the first and second reactions, calculate the equilibrium constant for CO2 (g) + H2(g) CH3OH(g) the third reaction. K, = 1.00× 105 co(g) + H2O(g) 2co(g) + H2(g) K2 3.74x 103
The synthesis of methanol from carbon monoxide and hydrogen gas is described by the following chemical...
The synthesis of methanol from carbon monoxide and hydrogen gas is described by the following chemical equation: CO(g)+2H2(g)⇌CH3OH(g)CO(g)+2H2(g)⇌CH3OH(g) The equilibrium constant for this reaction at 25 ∘C∘C is Kc=2.3×104Kc=2.3×104. In this tutorial, you will use the equilibrium-constant expression to find the concentration of methanol at equilibrium, given the concentration of the reactants. 1. a. Suppose that the molar concentrations for COCO and H2H2 at equilibrium are [CO][CO] = 0.04 MM and [H2][H2] = 0.04 MM. Use the formula you found...
5-3 Write the equilibrium constant expression of this reaction and calculate the concentration of all the...
5-3 Write the equilibrium constant expression of this reaction and calculate the concentration of all the gases at equilibrium for the reaction: CO(g) + H20 (g) = CO2(g) + H2 (g) Given that the initial concentrations of all the gases are 0.05 M and that Kc = 5.1 at 700 K.
Consider the chemical equation and equilibrium constant at 25°C: 2COF(g) = CO2(g) + CF4(g), K =...
Consider the chemical equation and equilibrium constant at 25°C: 2COF(g) = CO2(g) + CF4(g), K = 2.2 x 106 Calculate the equilibrium constant for the following reaction at 25°C: 2C02(g) + 2CF (g) = 4C0F2(g) Express the equilibrium constant to two significant figures.
When H2(g) is mixed with CO2(g) at 2,000 K, equilibrium is achieved according to the following...
When H2(g) is mixed with CO2(g) at 2,000 K, equilibrium is achieved according to the following equation CO2(g) + H2(g) « H2O(g) + CO(g) In one experiment, the following equilibrium concentrations were measured. [H2] = 0.20 mol/L [CO2] = 0.30 mol/L [H2O] = [CO] = 0.55 mol/L What is the mole fraction of CO(g) in the equilibrium mixture? Using the equilibrium concentrations given above, calculate the value of Kc, the equilibrium constant for the reaction. Determine...
Consider the balanced chemical equation for this equilibrium reaction: A (aq) + B (aq) = AB...
Consider the balanced chemical equation for this equilibrium reaction: A (aq) + B (aq) = AB (aq) To determine the equilibrium constant for this reaction at 298 K, a student mixes two solutions together and allows them to react: • 10.0 mL of 0.60 M A (aq), and, • 40.0 mL of 0.25 MB (aq). When this solution reaches equilibrium, the student measures the equilibrium concentration of AB in the 50.0 mL solution: [AB]E = 0.10 M. Which values should...
A.) Given the reaction 2A + B ⇋ 4 C (all gases) concentrations at equilibrium are...
A.) Given the reaction 2A + B ⇋ 4 C (all gases) concentrations at equilibrium are A = 0.076 M B = 0.829 M If K = 3.32, find the concentration of C and report it in M units. B.) Cu (s) + 2 Ag+ ⇋ Cu2+ (aq+) + 2 Ag(s) K = 7.88 x 104 PbCl2 (s) ⇋ Pb2+ (aq) + 2 Cl- (aq) K = 2.4 x 10-4 AgI (s) ⇋ Ag+ (aq) + I- (aq) K =...
Part A Calculate the equilibrium concentrations of CO2, H2, CO, and H.O at 298 Kif the initial concentrations are CO2-0.700 M and [H] -0.400 M The equilibrium constant for the reaction CO2(x) + H2(g) + CO(x) + H2O(R) is 9.71 x 10 at 298 K Express your answers in moles per liter to three significant figures separated by commas VO AE ? (CO, (H). (CO). [H0] M Denne
For the reaction N2(g) + 3H2(g) = 2NH3(g) what is the value of Ke at 500°C if the equilibrium concentrations are as follows: [H2] = 0.40 M, (N2) = 0.40 M, and (NH3) = 1.9 M Express the equilibrium constant to two significant figures. V AE OE ? Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining Set up the equilibrium-constant expression for this reaction using the equilibrium concentrations. The product concentrations a the reactant concentrations are...
Calculate Kc for the following reaction given the following
equilibrium concentrations of
H2(g) = 1.60 M CO(g) = .0030 M, and H2O(g) = 0.030 M. C(s) +
H2O(g) = CO(g) + H2(g)
(Hint: You DO include H2O(g) in the equilibrium expression)
K = ?
Save Answer Calculate K, for the following reaction given the following equilibrium concentrations of H2(9) = 1.60 M COO) = .0030 M, and H,00 = 0.030 M. Co+H,09 = COO + H2(9) (Hint: You Do include H,0...
Solve these two questions plz
ASAP
6. Consider the chemical equation and equilibrium constant for the synthesis of ammonia at 25 °C: Ng(g) + 3 H2(g-2NH3(g) K=3.7 x 108 Calculate the equilibrium constant for the following reaction at 25 C: 7. Given the equilibrium constants for the first and second reactions, calculate the equilibrium constant for CO2 (g) + H2(g) CH3OH(g) the third reaction. K, = 1.00× 105 co(g) + H2O(g) 2co(g) + H2(g) K2 3.74x 103
5-3 Write the equilibrium constant expression of this reaction and calculate the concentration of all the gases at equilibrium for the reaction: CO(g) + H20 (g) = CO2(g) + H2 (g) Given that the initial concentrations of all the gases are 0.05 M and that Kc = 5.1 at 700 K.
Consider the chemical equation and equilibrium constant at 25°C: 2COF(g) = CO2(g) + CF4(g), K = 2.2 x 106 Calculate the equilibrium constant for the following reaction at 25°C: 2C02(g) + 2CF (g) = 4C0F2(g) Express the equilibrium constant to two significant figures.
Consider the balanced chemical equation for this equilibrium reaction: A (aq) + B (aq) = AB (aq) To determine the equilibrium constant for this reaction at 298 K, a student mixes two solutions together and allows them to react: • 10.0 mL of 0.60 M A (aq), and, • 40.0 mL of 0.25 MB (aq). When this solution reaches equilibrium, the student measures the equilibrium concentration of AB in the 50.0 mL solution: [AB]E = 0.10 M. Which values should...
Most questions answered within 3 hours.
-
Let M = 8.00kg, m = 6.00kg, θ = 40.00, and the coefficient of
kinetic friction...
asked 3 minutes ago -
Java. For C through H True or false?
c. Primitive variables must be objects.
d. Integer...
asked 8 minutes ago -
Write a program that turns a 32-bit numeric value (e.g.,
0xFFFFh) and converts it to a...
asked 10 minutes ago -
A motor produces a torque of 0.25 N m at an angular velocity of
7200 revolutions...
asked 23 minutes ago -
***Please answer the below java question***
Are static methods inheritable? Can they be overridden?
asked 26 minutes ago -
In reaching her destination, a backpacker walks with an average
velocity of 1.13 m/s, due west....
asked 26 minutes ago -
Write two C programs that run a
server program and a client program concurrently.
Server program:...
asked 25 minutes ago -
Executive Program Practical Connection Assignment
Subject : Operations Security.
Assignment:
Provide a reflection of at least...
asked 35 minutes ago -
Every time Casey is at bat he has a 0.4 probability of
getting on base (assume...
asked 43 minutes ago -
The Walston Company is to be liquidated and has the following
liabilities:
Income taxes
$
9,400...
asked 50 minutes ago -
If
the more comprehensive data is available in MEPS, why does the NHIS
still exist? How...
asked 1 hour ago -
Koo argues that the Japanese economy in the 1990s suffered from
a balance sheet recession. What...
asked 1 hour ago