Homework Answers
I don´t know the reaction of part 3, but i assume it is:
C(s) + CO2(g) ----> 2CO(g)
When you change the amount of a reagent or product the reaction will try to restore the equilibrium. But, the value of Kp is always the same. The concentrations of product and reagents will change in order to achive a new situation in which the PCO2/PCO2 = Kp.
The only thing that changes Kp is temperature. So the correct answer is A.
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I need help with number 4
B. There are more reactants than products at equilibrium C....
A) No change in the equilibrium C) More information is needed to answer the question. B)...
A) No change in the equilibrium C) More information is needed to answer the question. B) Equilibrium shifts to the right. D) Equilibrium shifts to the left E) None of the answers is correct. Q(17) Which species is amphiprotic? A) H3PO B) H2PO D) None of these C) PO Q(18) Ni(CO)4)Nie)+ 4 COlaAdding nickel (solid) to this reaction will cause the equilibrium to A) Shift toward the products C) remain unchanged E) it depends on the amount added B) Shift...
Q(18) NI(CO)A(9) - Nica) + 4 CO)Adding nickel (solid) to this reaction will cause the equilibrium A) Shift toward...
Q(18) NI(CO)A(9) - Nica) + 4 CO)Adding nickel (solid) to this reaction will cause the equilibrium A) Shift toward the products B) Shift toward the reactants C) remain unchanged D) increase the temperature E) it depends on the amount added Q(19) CO2 + H2 -CO + H2O Adding a catalyst to this reaction will cause the (CO) at equilibrium to A) Shift toward the products B) Shift toward the reactants C) remain unchanged D) increase the temperature E) it depends...
Q(18) NI(CO)49) - Ni(s) + 4 CO(g)Adding nickel (solid) to this reaction will cause the equilibrium...
Q(18) NI(CO)49) - Ni(s) + 4 CO(g)Adding nickel (solid) to this reaction will cause the equilibrium to A) Shift toward the products B) Shift toward the reactants C) remain unchanged D) increase the temperature E) it depends on the amount added Q(19) CO2 + H2 -CO + H2O Adding a catalyst to this reaction will cause the COD at equilibrium to A) Shift toward the products B) Shift toward the reactants C) remain unchanged D) increase the temperature E) it...
Q(17) Which species is amphiprotic? A) H3PO4 C) PO43- D) None of these B) H2PO4 Q(18)...
Q(17) Which species is amphiprotic? A) H3PO4 C) PO43- D) None of these B) H2PO4 Q(18) Ni(CO)4(g)Nis)+ 4 CO(g)Adding nickel (solid) to this reaction will cause the equilibrium to C) remain unchanged E) it depends on the amount added B) Shift toward the reactants A) Shift toward the products D) increase the temperature Q(19) CO2 H2 CO + H20 Adding a catalyst to this reaction will cause the [CO] at equilibrium to A) Shift toward the products C) remain unchanged...
QUESTION 4 Which of the following statements about a system at chemical equilibrium is true? The...
QUESTION 4 Which of the following statements about a system at chemical equilibrium is true? The concentrations of the reactants and products remain constant. The concentration of products is always greater than the concentration of reactants. The concentration of products is always less than the concentration of reactants. There are no products formed. There are no more reactants left.
Chemical Equilibrium partial pressure Q1.) I need help with Part 2 on this problem Making CO...
Chemical Equilibrium partial pressure
Q1.) I need help with Part 2 on this
problem
Making CO from CO2 is a potential energy source. The value of Kp
for the reaction is is 1.50 at 700.0°C
CO2 (g) +C(s)
2CO(g)
Q2.)
Calculate the equilibrium partial pressure of CO if initially Pco2 1.29 atm and Pco 4.40 atm. Pure graphite is present initially and when equilibrium is achieved 1.94 atm Part 2 (1 pt) O See Hint Calculate the equilibrium partial pressure...
3a. Determine the equilibrium pressures of all the reactants and products for the equilibrium described below...
3a. Determine the equilibrium pressures of all the reactants and products for the equilibrium described below if you start with an initial pressure of carbon dioxide and carbon tetrafluoride each at 0.750 atm with no COF2 present. You can assume that the temperature is constant at 1550K. (12 points) 2COF2(g) CF4(g) + CO2(g) KP = 0.168 at 1550K Initial pressures: PCO2 = PCF4 = 0.750 atm; PCOF2 = 0.000 atm 3b. What is the value of KC for this reaction?...
1. 1.00 mole of gaseous methane was put into a 1.0L flask ad 483K. The equilibrium...
1. 1.00 mole of gaseous methane was put into a 1.0L flask ad
483K. The equilibrium mixture as depicted below was found. The
equilibrium constant, KC, is
CO(g) + 2H2(g)
CH3OH(g)
a) will be greater than 1 since products are favored
b) will be less than 1 since reactants are favored
c) neither statement above is correct because there are equal
amounts of reactants and products
2. For the reaction given below, the diagram represents an
equilibrium mixture. Calculate the...
A Which one of the following will change the value of an equilibrium constant? a) Varying the initial concentrations of...
A Which one of the following will change the value of an equilibrium constant? a) Varying the initial concentrations of reactants b) Varying the initial concentration of products c) Changing the volume of the reaction vessel d) Changing temperature e All of the above 5) The equililbrium constant for the gas phase reaction N2(g)+3H2(g) 2NH,(g) is Keg 4.34 x 10 at 300°C. At equilibrium a) products predominate b) only products are present reactants predominate d) only reactants are present roughly...
Select all of the true statements regarding chemical equilibrium. The concentrations of reactants and products are...
Select all of the true statements regarding chemical equilibrium. The concentrations of reactants and products are equal. The concentrations of reactants and products remain constant. Reactants are being converted to products and vice versa. The rates of the forward and reverse reactions are equal. Write the equilibrium constant expression for the reaction A(s)+3 B() 2C (aq) D(aq) in terms of [A]. [B]. [C], and [D] K = Write the equilibrium-constant expression for the reaction shown in terms of [A]. [B]....
A) No change in the equilibrium C) More information is needed to answer the question. B) Equilibrium shifts to the right. D) Equilibrium shifts to the left E) None of the answers is correct. Q(17) Which species is amphiprotic? A) H3PO B) H2PO D) None of these C) PO Q(18) Ni(CO)4)Nie)+ 4 COlaAdding nickel (solid) to this reaction will cause the equilibrium to A) Shift toward the products C) remain unchanged E) it depends on the amount added B) Shift...
Q(18) NI(CO)A(9) - Nica) + 4 CO)Adding nickel (solid) to this reaction will cause the equilibrium A) Shift toward the products B) Shift toward the reactants C) remain unchanged D) increase the temperature E) it depends on the amount added Q(19) CO2 + H2 -CO + H2O Adding a catalyst to this reaction will cause the (CO) at equilibrium to A) Shift toward the products B) Shift toward the reactants C) remain unchanged D) increase the temperature E) it depends...
Q(18) NI(CO)49) - Ni(s) + 4 CO(g)Adding nickel (solid) to this reaction will cause the equilibrium to A) Shift toward the products B) Shift toward the reactants C) remain unchanged D) increase the temperature E) it depends on the amount added Q(19) CO2 + H2 -CO + H2O Adding a catalyst to this reaction will cause the COD at equilibrium to A) Shift toward the products B) Shift toward the reactants C) remain unchanged D) increase the temperature E) it...
Q(17) Which species is amphiprotic? A) H3PO4 C) PO43- D) None of these B) H2PO4 Q(18) Ni(CO)4(g)Nis)+ 4 CO(g)Adding nickel (solid) to this reaction will cause the equilibrium to C) remain unchanged E) it depends on the amount added B) Shift toward the reactants A) Shift toward the products D) increase the temperature Q(19) CO2 H2 CO + H20 Adding a catalyst to this reaction will cause the [CO] at equilibrium to A) Shift toward the products C) remain unchanged...
QUESTION 4 Which of the following statements about a system at chemical equilibrium is true? The concentrations of the reactants and products remain constant. The concentration of products is always greater than the concentration of reactants. The concentration of products is always less than the concentration of reactants. There are no products formed. There are no more reactants left.
Chemical Equilibrium partial pressure
Q1.) I need help with Part 2 on this
problem
Making CO from CO2 is a potential energy source. The value of Kp
for the reaction is is 1.50 at 700.0°C
CO2 (g) +C(s)
2CO(g)
Q2.)
Calculate the equilibrium partial pressure of CO if initially Pco2 1.29 atm and Pco 4.40 atm. Pure graphite is present initially and when equilibrium is achieved 1.94 atm Part 2 (1 pt) O See Hint Calculate the equilibrium partial pressure...
1. 1.00 mole of gaseous methane was put into a 1.0L flask ad
483K. The equilibrium mixture as depicted below was found. The
equilibrium constant, KC, is
CO(g) + 2H2(g)
CH3OH(g)
a) will be greater than 1 since products are favored
b) will be less than 1 since reactants are favored
c) neither statement above is correct because there are equal
amounts of reactants and products
2. For the reaction given below, the diagram represents an
equilibrium mixture. Calculate the...
A Which one of the following will change the value of an equilibrium constant? a) Varying the initial concentrations of reactants b) Varying the initial concentration of products c) Changing the volume of the reaction vessel d) Changing temperature e All of the above 5) The equililbrium constant for the gas phase reaction N2(g)+3H2(g) 2NH,(g) is Keg 4.34 x 10 at 300°C. At equilibrium a) products predominate b) only products are present reactants predominate d) only reactants are present roughly...
Select all of the true statements regarding chemical equilibrium. The concentrations of reactants and products are equal. The concentrations of reactants and products remain constant. Reactants are being converted to products and vice versa. The rates of the forward and reverse reactions are equal. Write the equilibrium constant expression for the reaction A(s)+3 B() 2C (aq) D(aq) in terms of [A]. [B]. [C], and [D] K = Write the equilibrium-constant expression for the reaction shown in terms of [A]. [B]....
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