Problem 11 Consider the reaction: A (aq) + (aq) at 293 K where the initial concentration...
A student ran the following reaction in the laboratory at 293 K: 2CH2Cl2(g) CH4(g) + CCl4(g) When she introduced 6.91×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(g) to be 3.19×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc=?
Consider the reaction below. The initial concentration of KBr is 0.0183 M, and the initial concentrations of K+ and Br− are each 0 M. If the equilibrium constant is Kc=7.76 under certain conditions, what is the equilibrium concentration of KBr? KBr(aq)⇌K+(aq)+Br−(aq) Remember to use correct significant figures in your answer (round your answer to the nearest hundredth).
Consider the system: A(aq) B(aq) at 277 K where AGFormA = -14.3 kJ/mol and AG form B = -13.2 kJ/mol. Calculate the concentration of A at equilibrium when 1.7 mol of A and 1.58 mol of B are mixed in water to form exactly one liter of solution. concentration (M) = number (rtol=0.01, atol=1€ @
Consider the reaction. A ( aq ) ⇀ ↽2 B ( aq ) K = 1.24 × 10 − 6 at 500 K If a 1.70 M sample of A is heated to 500 K, what is the concentration of B at equilibrium?
Consider the system: A (aq) → B (aq) at 283 K where ΔGoform A = -18.3 kJ/mol and ΔGoform B = -17.3 kJ/mol. Calculate the concentration of B at equilibrium when 2.21 mol of A and 1.71 mol of B are mixed in water to form exactly one liter of solution.
Consider the reaction. A(aq) 3 B(aq) K - 7.29 X 10 at 500 K If a 3.10 M sample of A is heated to 500 K, what is the concentration of B at equilibrium? [B] =
Consider the system: A (aq) + B (aq) at 255 K where AG mA = -13.7 kJ/mol and AG B = -17.7 kJ/mol. Calculate the concentration of B at equilibrium when 2.36 mol of A and 1.01 mol of B are mixed in water to form exactly one liter of solution.
Consider the reaction. A(aq) = 2 B(aq) K = 3.52 x 10-6 at 500 K If a 4.10 M sample of A is heated to 500 K, what is the concentration of B at equilibrium? [B] = M
Consider the reaction. A(aq) = 3 B(aq) K. = 6.30 x 10-6 at 500 K If a 3.50 M sample of A is heated to 500 K, what is the concentration of B at equilibrium? [B] = M
Consider the reaction. A(aq) = 2 B(aq) K. = 4.22 x 10-6 at 500 K If a 5.00 M sample of A is heated to 500 K, what is the concentration of B at equilibrium? [B] = M