How many atoms of carbon are contained in 47.6 g of aluminum carbonate? The molar mass of aluminum carbonate is 233.99 g/mol. 1.23×1023 C atoms 2.96×1024 C atoms 2.87×1025 C atoms 3.68×1023 C atoms
The weight average molecular mass and the number average molecular mass of a polymer are 20,000 (Mw) and 30,000 (Mn), respectively. The polydispersity index is equal to: a. 2 b. < 1 c. > 1 d. 1.5 e. None of the above
1.6 mol of CH3OH (g) are injected into a 4.0 L container and the following equilibrium is established. 2H2 (g) + CO2 (g) ⇌ CH3OH (g) + 92 kJ a) At equilibrium, 0.80 mol of CH3OH is still in the container. Determine the equilibrium concentrations of all entities in mol/L. (4) b) Write the equilibrium law expression for this system. (1) c) Calculate the value of the equilibrium constant.
A gas sample of a compound weighing 34.3 g (MW: 70.2 g/mol ) at 127.2 C is converted to the liquid phase at 44.6 C. What amount of heat (in J) is required to perform this process? Tb = 114 C Hvap = 2.44 kJ/mol specific heat of the gas is 4.3 g/J∗mol specific heat of the liquid is 1.4 g/J∗mol
A gas mixture of N2 and H2 has a total pressure of 952.455 kPa and contains 11.3 mol of gas. If the partial pressure of N2 is 495.479 kPa, how many moles of H2 are in the mixture? 5.88 4.51 11.3 5.42 5.65
A 4.30 L container had 33.40 moles of N2O4 added to it. When equilibrium was established, the concentration of NO2 was found to be 2.67 M. What is Kc for the following reaction N2O4(g) ↔ 2NO2(g) 0.997 M 0.415 M 0.942 M 0.374 M 0.353 M 1.108 M
Consider the following reaction at 298 K. Zn2+(aq) + 2 Ag(s) → Zn(s) + 2Ag+(aq) Which of the following statements are correct? Choose all that apply. Ecello < 0 K < 1 n = 2 mol electrons The reaction is product-favored. ΔG∘ < 0
Use the following information to answer the next two questions. NH4+(aq) + H2O(l) → H3O+(aq) + NH3(aq) In a system at equilibrium, the concentration of the NH3(m) is 0.35 mol/L and the concentration of the NH4+(aq) is 0.25 mol/L. The pH of the NH4+(aq)/NH3(aq) solution is (4 mark)
Given the following equation: 4 NH3(g) + 5O2 (g) → 4 NO (g) + 6H2O (l) How many moles of NH3 is required to produce 35.1 grams of H2O? mol NH3
When 6.00 mol each of I2 (g), Br2 (g), and IBr (g) are placed in a 2.00 L vessel at constant temperature, they reach equilibrium according to the following equation: I2 (g) + Br2 (g) ⇌ 2 IBr (g) If Keq for this reaction is 0.683: a. Is this system at equilibrium? If not, which way will it shift to reach equilibrium? b. Determine the concentrations of all entities at equilibrium. Show all your steps.
The heat of vaporization of water (H2O) is 539.2 cal/g. How much energy in calories is absorbed when 94. g of water is vaporized? Be sure your answer has the correct number of significant figures. cal ×10
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2(g) ⇌ 2HI(g) Kc = 53.3 At this temperature, 0.500 mol of H2 and 0.500 mol of I2 were placed in a 1.00−L container to react. What concentration of HI is present at equilibrium?
Determine the amount, in mol, of each compound present in the sample based on the mass and molecular formula provided: a) 3.23×10−3 g of the amino acid glycine, C2H5NO2 Amount: mol b) 0.325 kg of the insecticide Paris Green, Cu4(AsO2)6(CH3 CO2)2 Amount: mol
Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel mixtures, releases oxygen gas on decomposition: 2H2O2(l) → 2H2O(l) + O2(g) ΔHrxn = −196.1 kJ Calculate the heat for the decomposition of 526 kg of H2O2. ×10 kJ (Enter your answer in scientific notation.)
Write the expression for the equilibrium constant Kp for the following reaction. Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH3)2 as (PNH3)2. If either the numerator or denominator is 1 , please enter 1 4 MnO2(s) ↔ 2 Mn2O3(s) + O2(g)