I keep getting this problem
wrong help please
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I keep getting this problem
wrong help please
At a certain temperature, the equilibrium constant for...
At a certain temperature, the equilibrium constant for the chemical reaction shown is 1.39 x 10-?....
At a certain temperature, the equilibrium constant for the chemical reaction shown is 1.39 x 10-?. At equilibrium, the concentration of AB is 2.425 M, the concentration of BC is 1.525 M, and the concentration of AC is 0.200 M. Calculate the concentration of B at equilibrium. AB(aq) + BC(aq) = AC(aq) + 2 B(aq) [B] = M
At a certain temperature, the equilibrium constant for the chemical reaction shown is 7.30×10−37.30×10−3. At equilibrium,...
At a certain temperature, the equilibrium constant for the chemical reaction shown is 7.30×10−37.30×10−3. At equilibrium, the concentration of AB is 1.8251.825 M, the concentration of BC is 1.4251.425 M, and the concentration of AC is 0.1100.110 M. Calculate the concentration of B at equilibrium. AB(aq)+BC(aq)↽−−⇀AC(aq)+2B(aq)
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Ke. 근...
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Ke. 근 4C(g) 23 3A(g)+2B(g) K= 1.53x 10 If, at this temperature, 1.30 mol of A and 4.00 mol of B are placed in a 1.00-L container, what are the concentrations of A, B, and C at equilibrium? Number Number Number
I've tried this a million times and I keep getting it wrong! The equilibrium constant for...
I've tried this a million
times and I keep getting it wrong!
The equilibrium constant for the chemical equation N2(g)+3H2(g)2NH3(g) s Kp = 4.46 at 197 degree C. Calculate the value of the K for the reaction at 197 degree C. Kc =
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant Kc. 3A...
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant Kc. 3A + 2B -><- 4C kc=3.13x10^29 If at this temperature, 2.50 mol of A and 3.70 mol of B are placed in a 1.00L container, what are the concentrations of A, B, C at equilibrium? I know the answer to B and C but system is keep telling me A is wrong The answer I have is [A]=0 <--- wrong [B]=2.033 <--- correct [C}=3.333 <----...
At a certain temperature, the equilibrium constant, Ke, for this reaction is 53.3. H,(g) +12(R) 근...
At a certain temperature, the equilibrium constant, Ke, for this reaction is 53.3. H,(g) +12(R) 근 2H1(R) K, 53.3 At this temperature, 0.700 mol of H2 and 0.700 mol of I2 were placed in a 1.00-L container to react. What concentration of Hl is present at equilibrium? Number
I keep getting the answer wrong please show steps! Part A The change in enthalpy (AH)...
I keep getting the answer wrong please show steps!
Part A The change in enthalpy (AH) for a reaction is -23.5 kJ/mol. The equilibrium constant for the reaction is 2.1x103 at 298 K What is the equilibrium constant for the reaction at 605 K? Express your answer using two significant figures. Submit Request Answer
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Ke! 3A(g)...
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Ke! 3A(g) +2B(g) = 40() K.=2.13 10" Wat this temperature, 1.90 mol of A and 3.60 mol of B are placed in a 1.00-L container, what are the concentrations of A, B, and C at equilibrium? Number (A)- O M Number Number (c)-
please help QUESTION 18 At a certain temperature the equilibrium constant, Kc, equals 0.11 for the...
please help
QUESTION 18 At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICI(g) = 12(g) + Cl2(g). What is the equilibrium concentration of Cl2 if 3.76 mol of 12 and 3.76 mol of Cl2 are initially mixed in a 4.0-L flask? *Please report 3 significant figures. Numbers only, No unit. No scientific notation.
I've tried calculating the mL and mols after balancing the equation but I keep getting it...
I've tried calculating the mL and mols after balancing the
equation but I keep getting it wrong. please help
Write the balanced chemical equation for the following acid and base reaction. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) H2S04(3q) + Na0H(aq) chemPad Help Greek 2SO4(aq) + 2NaOH(aq) -2H20(/) + Na2SO4(aq) Correct. Using the balanced reaction above, calculate the amount of 0.0024 M NaOH that would neutralize 22 mL of 0.0025 M...
At a certain temperature, the equilibrium constant for the chemical reaction shown is 1.39 x 10-?. At equilibrium, the concentration of AB is 2.425 M, the concentration of BC is 1.525 M, and the concentration of AC is 0.200 M. Calculate the concentration of B at equilibrium. AB(aq) + BC(aq) = AC(aq) + 2 B(aq) [B] = M
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Ke. 근 4C(g) 23 3A(g)+2B(g) K= 1.53x 10 If, at this temperature, 1.30 mol of A and 4.00 mol of B are placed in a 1.00-L container, what are the concentrations of A, B, and C at equilibrium? Number Number Number
I've tried this a million
times and I keep getting it wrong!
The equilibrium constant for the chemical equation N2(g)+3H2(g)2NH3(g) s Kp = 4.46 at 197 degree C. Calculate the value of the K for the reaction at 197 degree C. Kc =
At a certain temperature, the equilibrium constant, Ke, for this reaction is 53.3. H,(g) +12(R) 근 2H1(R) K, 53.3 At this temperature, 0.700 mol of H2 and 0.700 mol of I2 were placed in a 1.00-L container to react. What concentration of Hl is present at equilibrium? Number
I keep getting the answer wrong please show steps!
Part A The change in enthalpy (AH) for a reaction is -23.5 kJ/mol. The equilibrium constant for the reaction is 2.1x103 at 298 K What is the equilibrium constant for the reaction at 605 K? Express your answer using two significant figures. Submit Request Answer
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Ke! 3A(g) +2B(g) = 40() K.=2.13 10" Wat this temperature, 1.90 mol of A and 3.60 mol of B are placed in a 1.00-L container, what are the concentrations of A, B, and C at equilibrium? Number (A)- O M Number Number (c)-
please help
QUESTION 18 At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICI(g) = 12(g) + Cl2(g). What is the equilibrium concentration of Cl2 if 3.76 mol of 12 and 3.76 mol of Cl2 are initially mixed in a 4.0-L flask? *Please report 3 significant figures. Numbers only, No unit. No scientific notation.
I've tried calculating the mL and mols after balancing the
equation but I keep getting it wrong. please help
Write the balanced chemical equation for the following acid and base reaction. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) H2S04(3q) + Na0H(aq) chemPad Help Greek 2SO4(aq) + 2NaOH(aq) -2H20(/) + Na2SO4(aq) Correct. Using the balanced reaction above, calculate the amount of 0.0024 M NaOH that would neutralize 22 mL of 0.0025 M...
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