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Problem- Determine the number of fundamental particles present in 54.341 g of Li2SO4. Properly include molecules or formula units in your answer.
Please be very comprehensive in your answer and do not omit any steps
calculate the pH of a buffer solution made by adding 10.0g of anhydrous sodium acetate (NaC2H3O2) to 100 ml of 0.100M acetic acid. sume there is no change in volume on adding the salt to the acid.
During mixing, heat is lost to the surroundings at a rate of 30 kJ s-1. What is the temperature of the warm water stream? Assume the specific heat of the water constant at 4.18 kJ kg-1 K-1.
A student used 40.5mL of 0.48M sodium carbonate solution and 45.6mL of the hydrochloric acid solution. The substance in the beaker at the end of the experiment had a mass of 0.93g. Calculate the concentration of the hydrochloric acid solution.
When 56.0 g calcium and 34.7 g nitrogen gas undergo a reaction that has a 88.0% yield, what mass of calcium nitride forms?
100 mL of 0.150 M acid H2A are mixed with 100 mL of 0.340 M NaOH. Calculate the [H+] of the resulting solution at equilibrium. Ka1 = 1.0 x 10^-5 Ka2 = 1.0 x 10^-7
What are the mole fractions of ethanol, C2H5OH, and water in a solution prepared by mixing 55g of ethanol with 45g of water
Give the formula of the conjugate base of the following Bronsted-Lowry acids. Explain your reasoning. Consider the substances GeH4, and SnH4
when 8.00g of NaOH is added to a calorimeter filled with 75.0mL of HCl the temperature of the solution increases for 25.0 C to 33.5 C. calculate the molar heat of neutralization for the NaOH. (assume that the density of the solution is 1.00gmL)
An unknown metal m reacts with sulfur to form a compound with the formula M2S3. If 3.12g of m reacts with 2.88g of S, what are the names of M AND M2S3
Calculate C (vm) i.e constant molar volume heat and the final pressure of a sample of carbon dioxide that expands reversibly and adiabatically from 57.4 kPa and 1 dm^3 to a final volume of 2 dm^3 . Take gamma(γ)= 1.4
A 25.00mL portion of 0.00923M NaOH (MM 40.00g/mol) was introduced into the solution of H2SO4 (MM 98.08g/mol), then the excess was back titrated with 13.33mL of 0.01007M HCl (MM 36.46g/mol). Calculate the parts per million of sulfur in the sample.
The annual production of zinc sulfide (ZnS) is 3.5 10^4 tons. Estimate the number of tons of SO2 produced by roasting it to extract zinc metal.
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