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A sample of a gas originally at 29°C and 1.25 atm pressure in a 3.0 L container is allowed to contract until the volume is 2.2 L and the temperature is 11°C. The final pressure of the gas is __________ atm.
a sample of nitrogen gas kept in a container of vulume 2.43 L and temp 27degree C exerts a pressure of 4.83 atm. calculate the number of moles of gas present
Determine the empirical formula of each of the following compounds. (Type your answer using the format CH4 for CH4 and list the elements in the same order as they are mentioned in the problem.
what is the freezing pint of a solution when 13.55 g of Mg(NO3)2 is dissolved in 156 mL of water when Tdegree
insulin is a protein that is used by the body to regulate both carbohydrate and fat metabolism. A bottle contains 475 of insulin at a concentration of 30.0 . What is the total mass of insulin in the bottle?
Solid copper (II) hydroxide from copper nitrate. First, add 30 mL of 3.0M sodium hydroxide to the solution in the Erlenmeyer Flask.Take a stirring rod and place the end about 1 cm into the solution; then tough the end to a 2 cm piece of red litmus..
A gas stream that contains 1.50 mole% CO2 flows through a pipeline. 20.0 kg/min of CO2 is injected into the line. A sample of the gas is drawn from a point in the line 10 meters downstream of the injection point and found to contain 2.3 mole% CO2.
Hard water contains alkaline earth cations such as Ca2+ which reacts with CO32- to form insoluble deposits of CaCO3. Will a precipitate of CaCO3 form if a 250mL sample of hard water having [Ca2+] = 8.0x10-4M is treated with the following
The solubility product constant of calcium sulfate,CaSO2 is 7.10*10^-5 . How many grams of calcium sulfate can dissolve in 53.5 of pure water
Calculate the mass of ethylene glycol required to lower the freezing point of 200 mL of water/ice by 4.5 degrees celsius. The K(f) for H20 is 1.86 degrees celsius/m. Assume the density of water is 1.00 g/ml.
An element has two isotopes with masses of 62.9396 u and 64.9278 u,and 30.83% of the atoms are the heavier isotope. Calculate the atomic mass of this element and give its name and symbol.
calculate the amount of heat transferred when 46.0 g of {rm{CH}}_3 {rm{OH}}(g) is decomposed by this reaction at constant pressure.
How much stomach acid was neutralized by the 4.3628 g tablet. How much stomach acid would have neutralized by the original 5.6831 tablet
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