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A metal sample weighing 124.10g and at a temperature of 99.3°C was placed in 42.87g of water in a calorimeter at 23.9°C. At equilibrium the temperature of the water and metal was 41.6°C. a) what was the ?t for the water? b) what was the ?t for the metal? c) how much heat flowed into the water? d) taking the specific heat of water to be 4.18J/g°C, calculate the specific heat of the metal? e) what is the approximate molar mass of the metal?
a couple drops of phenophalein indicator and then was titrated with 8.1mL of NaOH until it turned pink. what is the concentration of NaOH?
write equations for the chemical reactions that occurred between the aqueous solutions of the oxides of sulfur and calcium and between the aqueous solutions
what is the presentage compostition of both of the components, which is the limiting reagent (if there is) and what is the theoretical yeild of each of them.
Explain why it is important that the glassware and reagents used in a Grignard reaction are completely dry. Write an equation that describes what happens if phenylmagnesium bromide reacts with water.
What is the mass (in grams) of the precipitate when 8.05 g of barium nitrate reacts in solution with excess sodium carbonate
If the partial pressure of a gas produced in a reaction was determined to be 0.35 atm in a 161.0 mL container and at a temperature of 25.0°C, how many moles of gas were produced? (Hint: Use the ideal gas law and convert temperature to Kelvin, volu..
Carbon dioxide makes up approximately 0.04% of Earth's atmosphere. If you collect a 2.8 sample from the atmosphere at sea level (1.00 ) on a warm day (28), how many molecules are in your sample
Describe an electrochemical cell for which the following are the cell reactions. (A cell description includes the physical description of the anode and anode compartment with dissolved species,
A 25.0-mL sample of 0.100 M propanoic acid (HC3H5O2, Ka = 1.3 10-5) is titrated with 0.100 M NaOH solution. Calculate the pH after the addition of the following amounts.
A student adds 0.1 mol of oxalic acid (H2C2O4) and 0.1mol of sodium dihydrogen phosphate to enough water to make 1.0L of solution. The following equilibrium is established with Kc from this reaction greater than 1
How much energy (heat) is released when 1.9 moles of H2 reacts with 0.7 moles of Cl2 to create HCl(g) if the ΔHrxn = -184.6 kJ.
A buffer solution is composed of 1.360 g of KH2PO4 and 5.677 g of Na2HPO4. What is the pH of the buffer solution?
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