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Q1. What is the mass number of an iron atom that has 28 neutrons?
Q2. Calculate the number of neutrons of 239Pu.
Q3. Write the appropriate symbol for each of the following isotopes: (a) Z= 11, A= 23; (b) Z= 28, A= 64
Q4. Define, with two examples, the following terms: (a) alkali metals, (b) alkaline earth metal, (c) halogens, and (d) noble gases.
Q5. Identify the following as elements or compounds: (a) NH3, (b) N2, (c) CO, (d) Co, and (e) He.
Draw all possible resonance structures and label if they are minor, major resonance contributors and draw the resonance hybrid.
Metabolic reactions are regulated by a variety of regulatory mechanisms. Mention and discuss five mechanisms. Give clear examples of each.
an experiment requires 44.0 g of ethylene glycol a liquid whose density is 1.114 gml. rather than weigh the sample on a
molecular equation, complete ionic equation, and net ionic equation for: Sodium carbonate + sulfuric acid Cadmium chloride + sodium hydroxide Hydrochloric acid + sodium hydroxide Ammonium chloride + sodium hydroxide Sodium acetate + sodium hydroxi..
What is the maximum mass of aluminum chloride that can be formed when reacting 29.0g of AL with 34.0g of Cl
What is the molarity of the resulting solution when 20.0 mL of a 2.00 M aqueous solution is diluted by the addition of 30.0 mL of water
Identify the limiting reagent and the volume of CO2 formed when 11L CS2 reacts with 18L O2 to produce CO2 gas and SO2 gas at STP.
Calculate the ph of the solution made by adding 0.50mol of HOBr and 0.30 mol of KOBr to 1.00 L of water. The value of Ka for HOBr is 2.0 x 10^-9.
The first-order rate constant for the reaction of methyl chloride (CH3Cl) with water to produce methanol (CH3OH) and hydrochloric acid (HCl) is 3.32 10-10s-1 at 25°C. Calculate the rate constant at 38°C if the activation energy is 116 kJ/mol.
calculate the ph of buffer solution made from .20 M HC2H3O2 and .050 M C2H3O2 that has an acid dissociation constant for HC2H3O2 of 1.8*10-5.
What temperature is needed to double the equilibrium constant from its value at 298 K? What temperature is needed to increase the equilibrium constant by a factor of 10? What if the standard enthalpy change were 20.0 kJ?
What will the pH be if 0.910 g of NaOH (40.00 g/mol) is added to 500.00 mL of a 0.500 M acetic acid/acetate buffer with an initial pH of 4.59? The Ka for acetic acid is 1.8 x 10-5.
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