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1.250 g mass of standard aspirin is dissolved in approximately 20mL of 1 M NaOH. This solution is added to a 250-mL volumetric flask as well as diluted to the mark with DI water. Explain how many grams per mL of aspirin are in the resulting solution. Note a 250-mL volumetric flask has a precision of 0.01 mL as well as the amount of NaOH added has no bearing on the important figures in the final concentration).
Use the following rate constant equations to determine the equillibrium constant for the following reaction at 400 K, 600 K, 800 K.
A rigid tank with a volume of 2.5 m3 contains 15 kg of saturated liquid-vapor mixture of water at 75 0C . The water is heated. Determine the temperature at which the liquid in the tank is completely vaporized.
Chlorine trifluoride is used in processing nuclear reactor fuel. It has a vapor pressure of 29.1 torr at -47.0°C and its heat of vaporization is 30.61 kJ/mol.
In a certain decomposition reaction, dinitrogen pentoxide decomposes to form nitrogen dioxide gas and oxygen gas. It was found that at 187 seconds the concentration of oxygen gas was 0.374 mol/L and at 549.5 seconds the concentration of oxygen gas..
A mixture of .148 moles of C is reacted with .117 moles of O2 in a sealed 10L container at 500K producing CO and CO2. The total pressure is .640 atm. What is the partial pressure of CO?
what is the final temprature of 0.1222 mol of a perfect monatomic gas that preform 75 j of work adiabatically if the
A concentration cell is built based on the following half reaction by using two pieces of zinc as electrodes (each weighing 100.0 g), two Zn2+ solutions
The resulting solution required 13.73 mL of 0.176 mol L?1 NaOH(aq) to neutralize the excess, unreacted HCl. What was the percentage by mass of Mg(OH)2 in the original sample [Hint: When Mg(OH)2 or Al(OH)3 reacts with HCl(aq), the products are a ch..
A student measures the standard enthalpy change for reaction (C2H4(g) + H2O(g) CH3CH2OH(g)) to be -52.8 kJ :Calculate the standard enthalpy of formation.
To what volume should you dilute 95mL of a 12.0M H2SO4 solution to obtain 1.80M H2SO4 solution
Calculate the Z for the fourth ionization of Ti when it requires 425.6 kJ of energy to ionize 0.185 moles of Ti^3+ to Ti^4+ ( The electron being removed is in the outermost valence orbital of Ti^3+ ground state, therefore n = 3)
A sample of nitrogen gas kept in a container of volume 2.9 L and at a temperature of 39°C exerts a pressure of 4.7 atm. Calculate the number of moles of gas present
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