20. mol H2 reacts with 8.0 mol O2 to produce H2O. Determine the number of grams reactant in excess and number of grams H2O produced. Identify the limiting reactant. 8.1 g H2 , 2.9 x 102 g H2O 17. How many litres of O2 gas are required to produce 100. g Al2O3?
There will have some error. 2) A volatile liquid was allowed to evaporate in a 43.298 g flask that has a total volume of 252 ml. the temperature of the water bath was 100˚C at the atmospheric pressure of 776 torr. The mass of the flask and condensed vapor was 44.173 g. calculate the molar mass of the liquid. T = 273 + 100 = 373 V = 252 mL = 1 L / 1000 mL = 0.252 L P = 776 Torr R= 0.0821 mass of 44.173 - 43.298 g = 0.875g moles of gas = PV / RT = 776 x .252 / 62.363 x (273+100) =0.00841 moles molar mass = 0.875g / 0.00841 moles = 104.1 g/
1 mole of water B. 2 moles of water C. 3 moles of water D. 2 moles of water with 1 mole of hydrogen left over 8. Ten kilograms of hydrogen gas (H2) are mixed with 355 kg of chlorine (Cl2) in a 0.50 m3 drum. The two gases react to produce hydrogen chloride. What is the final pressure in the drum if the final temperature is 60oC?
If the gases in the can reach a pressure of 90 lbs/in2, the can will explode. To what temperature must the gases be raised in order for the can to explode? Assume constant volume. (630 oC) 7. Maybelline Cousteau’s backup oxygen tank reads 900 mmHg while on her boat, where the temperature is 27oC.
An exhaled air bubble underwater at 290. kPa has volume 18.9 mL. What will be its volume at the water’s surface where the pressure is 104 kPa. (Why must a diver exhale during ascent?) P 2 3. What pressure is required to reduce the volume of gases in a car’s cylinder from 48 cm3 at V1 102 kPa to 5.2 cm3?
Percent H2O in Hydrate is equal 0.34/2.33=14.6% 3. The general formula of barium chloride hydrate is BaClg-nHZO, where n is the number of water molecules. Calculate the theoretical percent water for each value of n—divide the sum of the atomic masses due to the water molecules by the sum of all the atomic masses in the hydrate, and multiply the result by 100. Complete the table. | BaCl2 | BaCl2•H2O | BaCl2•2H2O | BaCl•3H2O | Sum of atomic masses (BaCl2) | 208.23 | 208.23 | 208.23 | 208.23 | Sum of atomic masses (nH2O) | 0 | 18.02 | 36.04 | 54.06 | Sum of atomic masses (hydrate) | 208.23 | 226.25 | 244.27 | 262.29 | Percent water in hydrate (theoretical) | 0% | 7.96% | 14.75% | 20.61% | In this lab we used a Balance, centigram
Answer is: the roof 13.What is the deepest lake in the world, and where is it located? * Answer: is: Caspian sea it is located in Asia- Europe 14.What is “brackish water”? Answer is: a mixture of seawater and freshwater 15. How many inches of rain does the tropical rain forest receive? Answer is: 50 to 260 inches »»»»When you see an asterisk (*), next to the answers for number 9 and 13, make sure you look on the left hand side of the webpage for an
Solution Stoichiometry and Gas Law Problems Problem 1 In flask A, 1.500g of silver nitrate solid is dissolved in 50.0mL of water, while in flask B, 0.500g of potassium carbonate is dissolved in 25.0mL of water. The two solutions are then mixed together. a) Before mixing, what is the molarity of each solution? b) Write the balanced molecular equation, the complete ionic equation, and the net ionic equation for the reaction. c) If the percentage yield is 85.0%, what mass of precipitate is actually produced?
How many kilograms of pure HCl would be used to make this hydrochloric acid? (Assume that 30% has two significant figures. There are 2000 lb/ton.) (Obj 15) 30 ton HCl 2000 lb 1 kg ? kg HCl = 6.0 × 105 ton HCl soln 100 ton HCl soln 1 ton 2.205 lb 30 ton HCl 2000 lb 453.6 g 1 kg ?
To do that we had to count the molar mass (M) of zinc sulfate. Then we multiplied the amount of zinc sulfate in moles with the molar mass. Then the answer was the mass (m) of the zinc sulfate to add in grams. M(ZnSO4) = (65.38 + 32.06 + 4 x 16.00) g/mol = 161.44 g/mol n (ZnSO4) = 0.02 mol M (ZnSO4) = 161.44