A 60.0 g sample containing mixed BaO and CaO are transformed into mixed sulfates weighing 10.34 grams. Calculate the percentage BaO and CaO in the sample.
Bao= x* 153.3
Cao= y*56.0779
x*153.3g + y*56.0774=10.34g
x*233.38g + y*136.14=60.00g
x=126.744 molBao
y= 185.8 molCao
A 60.0 g sample containing mixed BaO and CaO are transformed into mixed sulfates weighing 10.34...
A 0.6407 g sample containing chloride and iodide ions gave a silver halide precipitate weighing 0.4430 g. This precipitate was then strongly heated in a stream of Cl2 gas to convert the AgI to AgCl; on completion of this treatment, the precipitate weighed 0.3181 g. Calculate the percentage of chloride and iodide in the sample separately.
If a 61 g sample of metal at 100oC is placed into a calorimeter containing 60.0 g of water at 18.0 oC, the temperature of the water increases to 22.0 °C. Calculate the amount of heat lost by the metal sample in calories.
A sample of a chromium-containing alloy weighing 3.450 g was dissolved in acid, and all the chromium in the sample was oxidized to 2CrO42–. It was then found that 3.18 g of Na2SO3 was required to reduce the 2CrO42– to CrO2– in a basic solution, with the SO32– being oxidized to SO42–. Write a balanced equation for the reaction of 2CrO42– with SO32- in a basic solution. Please include physical states! How many grams of chromium were in the alloy...
You placed 6.35 g of a mixture containing unknown amounts of BaO(s) and MgO(s) in a 3.50-L flask containing CO₂(g) at 30.0°C and 750. torr. After the reaction to form BaCO₃(s) and MgCO₃(s) was completed, the pressure of CO₂(g) remaining was 135 torr. Calculate the mass of BaO(s) in the mixture.
A metal sample weighing 24.000 g is heated to 100.0 degrees celsius and then transferred into a calorimeter containing 30.0 mL of water at a temperature of 22.8 degrees celsius. If the specific heat of the metal is 0.105 J/g*C, what is the final temperature of the metal sample plus water?
a solution containing 2.35 g of sodium carbonate is mixed with one containing 12.8 g of silver nitrate write the balanced equation balance the molecular equation write the net ionic equation determine the limiting reactant calculate the amount of silver carbonate formed
10. A sample weighing 106.7 grams is analyzed and found to contain 42.97 g of potassium, 28.57 g of chromium; the remainder is oxygen. What is the empirical, or simplest, formula of this substance? 1027 11·An organic compound is analyzed and found to be 38.71 % carbon and 9.68 % hydrogen; the rest is oxygen. If the molecular weight of this substance is 62 g/mol, what is the molecular formula of this substance? 12. A sample weighing 112.2 grams is...
A 23.28mL solution containing 1.684 g Mg(NO3)2 is mixed with a 31.67mL solution containing 1.172 g NaOH. Calculate the concentrations of the Na + and NO3- ions that remain in solution. Assume volumes are additive. Balanced equation not needed to solve the problem.
A 21.524 g paint sample was analyzed for barium (Ba2+, MW = 137.327 g/mole) by an EDTA back titration: Ba2+(aq) + Y4–(aq) à BaY2–(aq). The sample was dissolved in acid and sufficient water was added to produce a volume of 100 mL. 10.00 mL of this concentrated solution was diluted to a volume of 50.00 mL. 25.00 mL of the diluted solution was treated with 33.95 mL of excess 0.09456 M EDTA. The excess EDTA was titrated to the endpoint...
A 32.0-g sample of an unknown metal at 99°C was placed in a constant-pressure calorimeter containing 60.0 g of water at 24.0°C, The final temperature of the system was found to be 28.4℃ Calculate the specific heat of the metal. (The heat capacity of the calorimeter is 14.4/C) J/g °C