Calculate M/MS for a paramagnet with J=7/2 at 85.0 °C and 0.400 T
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A 20.0-mL sample of 0.400 M HBr solution is titrated with 0.400 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added. (a) 11.6 mL (b) 15.7 mL (c) 20.0 mL (d) 28.2 mL (e) 33.1 mL
A closed surface with dimensions a = b = 0.400 m and c = 0.800 m is located as shown in the figure below. The left edge of the closed surface is located at position x = a. The electric field throughout the region is non- uniform and given by E = [(5.00xy)i + (5.00x2y)j ] N/C, where y is in meters. 3) Calculate the net electric flux leaving the closed surface. 4) What net charge is enclosed by the...
Calculate the solubility (in g/L) of CaSO 4 ( s ) in 0.400 M Na 2 SO 4 ( aq ) at 25 ° C . The K sp of CaSO 4 is 4.93 × 10 − 5 .
1. Calculate the [H3O+] and pH of the following polyprotic acid solution: 0.400 M H3PO4. Calculate the pH of this solution. 2. Calculate the [H3O+] and pH of the following polyprotic acid solution: 0.400 M H2C2O4.
Calculate final temp of water when a 3.00 g piece of iron at 85.0°C (Specific heat 0.45 J/g °C; density = 7.05 gmL ) is added to 35.0 mL of water (initial temp is 22.5°C) Density of water. 1.00g/mL; Specific heat of water: 4.18 J/g oC
The rate constant for this second-order reaction is 0.400 M-'.5' at 300 °C. A products How long, in seconds, would it take for the concentration of A to decrease from 0.770 M to 0.360 M? R. T U T O P F G H J K L NM <
4. A 202. gram sample of copper (C =0.20 j/g-deg. C) is heated to 85.0 deg. C and then placed in a container of 100.0 grams of water at 19.2 deg. C. What is the final temperature of the system?
Experiment auw. [A] (M) 0.100 0.100 0.100 0.200 0.300 0.400 [B] (M) 0.100 0.200 0.400 0.400 0.500 0.500 Rate (M/s) 0.0101 0.0403 0.162 0.323 0.485 0.646 Question 5 of 7 3 Points Which of the following is the correct unit for the rate constant in the question O A.M ^_151-1 OB.M^-251-1 OC. M^1 S-1 OD. M^2 S11 Reset Selection
100.0 mL of 0.400 M aqueous NaOH and 50.00 mL of 0.400 M aqueous H2SO4, each at 24.00°C, were mixed, see equation: 2NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l) The final temperature achieved by the solution was 26.65 °C. Neglect the heat capacity of the cup and the thermometer, and assume that the solution of products has a density of exactly 1.00 g/mL and specific heat capacity of 4.18 J/(g•C) How much heat did the reaction release?
A mixture initially contains A, B, and C in the following concentrations: [A] = 0.400 M , [B] = 1.20 M , and [C] = 0.700 M . The following reaction occurs and equilibrium is established: A+2B⇌C At equilibrium, [A] = 0.260 M and [C]= 0.840 M . Calculate the value of the equilibrium constant, Kc.