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A 1.75L container contains 32.5 mol of Xe at 75oC. Compute the pressure of the gas (a) assuming ideal gas behavior also (b) using the Vander Waals equation. For Xe, a = 4.194 L2atm/mol2 and b = 0.05105 L/mol.
a mole of atoms ions molecules or anything else contains avogadros number 6.022 x 1023 of these units. a mole of
A catalyst may be defined as a substance that enhances the rate of a chemical reaction without being consumed in the process. By this definition, a catalyst would have an infinite lifetime. The ozone decomposition catalysts
What is the pH of a solution containing 0.10 L of 0.10 M acetic acid, to which 0.010 moles of acetate are added. Volume does change in this case. Density of the acetate salt is 55.05 g/mL
What would happen to the calcium ion concentration in a saturated solution of Ca(OH)2 if the hydroxide ion concentration is increased by dissolving solid NaOH. What is the name of this effect
Heating any of the three isomeric dimethylbenzenes with HF in the presence of BF3 to 80 C leads to the equilibrium mixture shown below: 1,2-Dimethylbenzene: 18% , 1,3-Dimethylbenzene: 58% , 1,4-Dimethylbenzene: 24%
When 189.4 g of ethylene (C2H4) (molar mass= 28.05 g/mol) burns in oxygen to give carbon dioxide and water, how many grams of CO2 (molar mass= 44.01 g/mol) are formed? C2H4 + 3O2 --> 2 CO2 + 2H2O
write balanced molecular ionic and net ionic equations for the reactions of chromium gives cr3 with solution of dilute
Write the balanced chemical equation that corresponds to this reaction. B) If 15g cyclohexane is burned in a calorimeter with a heat capacity of 230kJ/K, what temperature change do you expect
2NO (g)+ Br2 (g) yields 2NOBr (g) What is the rate of disappearance of Br2 when [NO]= 5.9×10-2 M and [Br2] = 0.26 M
If the partial pressure of H2S is 0.539 atm, calculate the total pressure (atm) of the mixture visualized. I wasn't able to put the actual visualization but I will provide to the best of my ability what was given
A sample of 1.42 g of Helium and an unweighed quantity of Oxygen are mixed in a flask at room temperature. The partial pressure of Helium is 42.5 torr and of oxygen is 158 torr.
Sulfuric acid sold for laboratory use consists of 96.7% by mass sulfuric acid; the rest is water. the density of the solution is 10845 g.cm^(-3). Compute the number of kg and pounds of sulfuric acid in 2.20 liter bottle of laboratory sulfuric acid
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