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LULUI Question 4 of 10 4. If Q is less than K, the ratio of products...
The equilibrium constant () of the reaction below is K-6.0 x 10 with initial concentrations as...
The equilibrium constant () of the reaction below is K-6.0 x 10 with initial concentrations as follows: [H2] = 1.0 x 102 M. [Na] - 4.0 M, and (NH) - 1.0 x 10* M. N (8) + 3H,() 2NH3(e) 3. Consider the chemical reaction: N2 + 3H2 yields 2NH3. If the concentration of the reactant Hy was increased from 1.0 x 10-2M to 2.5 x 10-M, calculate the reaction quotient (C) and determine which way the chemical system would shift...
The Reaction Quotient 9 of 10 > - Review Constants Periodic Table When conducting chemical reactions...
The Reaction Quotient 9 of 10 > - Review Constants Periodic Table When conducting chemical reactions in the lab or in industrial processes, it can be important to know whether a reaction has reached equilibrium By measuring the reaction quotient, Q. of a chemical reaction and comparing it to the equilibrium constant, K, we can identify whether a reaction is at equilibrium Correct Q is less than K, the ratio of products to reactants is smaller than at equilibrium. In...
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) +...
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + O2(g) ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M 2. The reaction below is not at equilibria and Q = 1.7. The equilibrium constant is K = 0.230. 2SO3(g) ⇌ 2SO2(g) + O2(g)...
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.
did i do this correctly ? Prediction, 1 • H2(g) + 12(g) = 2HI(g) K =...
did i do this correctly ?
Prediction, 1 • H2(g) + 12(g) = 2HI(g) K = 64.0 • a mixture has the following concentrations: - [12]o = 1.0 M, [Hz]. = 1.0 M, and [HI]. = .1 M. - a. Is the system at equilibrium? - A. YES B. NO - If not, what change occurs? - A. shift to right B. shift to left Predictions WI Q and K 1) H2 (9) + I219) = 2111910 - [In]:10M (H2)...
Review Constants Periodic Table When conducting chemical reactions in the lab or in industrial processes, can...
Review Constants Periodic Table When conducting chemical reactions in the lab or in industrial processes, can be important to know whether a reaction has reached equilibrium. By measuring the reaction quotient, Q. of a chemical reaction and comparing it to the equilibrium constant, K. we can identity whether a reaction is at equilibrium ✓ Correct Q is less than K. the ratio of products to reactants is smaller than at equilibrium. In this case, the reaction wil proceed to the...
N2(g) + O2(g) equilibrium reaction arrow 2 NO(g); Kc = 5.6 ✕ 10−4 at 2098 K...
N2(g) + O2(g) equilibrium reaction arrow 2 NO(g); Kc = 5.6 ✕ 10−4 at 2098 K (a) What is the value of Kc for the reaction 2 NO(g) equilibrium reaction arrow N2(g) + O2(g) at the same temperature? (b) What is the value of Kc for the reaction 1/2 N2(g) + 1/2 O2(g) equilibrium reaction arrow NO(g) at the same temperature? (c) Does the equilibrium in (a) favor the reactant or the products? reactant products (d) Does the equilibrium in...
please show all work Question 45 2 pts What is the total internal energy change (AE),...
please show all work
Question 45 2 pts What is the total internal energy change (AE), in kJ, of a system that absorbs 15.4 kJ of heat and does 21.40 kJ of work on the surroundings? O 6.0 O 36.8 -36.8 O-6.0 Question 46 2 pts What is the conjugate base of HSO4? HSO4 H2SO4 O S042 H2SO4 Given the partial pressures and concentrations for the reactants and products below, answer questions 47-49. C2O 2 HF 2F( H2C204 ( (ag)...
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...
The equilibrium constant () of the reaction below is K-6.0 x 10 with initial concentrations as follows: [H2] = 1.0 x 102 M. [Na] - 4.0 M, and (NH) - 1.0 x 10* M. N (8) + 3H,() 2NH3(e) 3. Consider the chemical reaction: N2 + 3H2 yields 2NH3. If the concentration of the reactant Hy was increased from 1.0 x 10-2M to 2.5 x 10-M, calculate the reaction quotient (C) and determine which way the chemical system would shift...
The Reaction Quotient 9 of 10 > - Review Constants Periodic Table When conducting chemical reactions in the lab or in industrial processes, it can be important to know whether a reaction has reached equilibrium By measuring the reaction quotient, Q. of a chemical reaction and comparing it to the equilibrium constant, K, we can identify whether a reaction is at equilibrium Correct Q is less than K, the ratio of products to reactants is smaller than at equilibrium. In...
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.
did i do this correctly ?
Prediction, 1 • H2(g) + 12(g) = 2HI(g) K = 64.0 • a mixture has the following concentrations: - [12]o = 1.0 M, [Hz]. = 1.0 M, and [HI]. = .1 M. - a. Is the system at equilibrium? - A. YES B. NO - If not, what change occurs? - A. shift to right B. shift to left Predictions WI Q and K 1) H2 (9) + I219) = 2111910 - [In]:10M (H2)...
Review Constants Periodic Table When conducting chemical reactions in the lab or in industrial processes, can be important to know whether a reaction has reached equilibrium. By measuring the reaction quotient, Q. of a chemical reaction and comparing it to the equilibrium constant, K. we can identity whether a reaction is at equilibrium ✓ Correct Q is less than K. the ratio of products to reactants is smaller than at equilibrium. In this case, the reaction wil proceed to the...
please show all work
Question 45 2 pts What is the total internal energy change (AE), in kJ, of a system that absorbs 15.4 kJ of heat and does 21.40 kJ of work on the surroundings? O 6.0 O 36.8 -36.8 O-6.0 Question 46 2 pts What is the conjugate base of HSO4? HSO4 H2SO4 O S042 H2SO4 Given the partial pressures and concentrations for the reactants and products below, answer questions 47-49. C2O 2 HF 2F( H2C204 ( (ag)...
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...
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Caculate the PH THANK YOU!
[OH−] = 1.9×10−7 M
[OH−] = 1.6×10−8 M
[OH−] = 7.2×10−11...
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