Calculate the volume of 0.250 M H2SO4 that contains 0.250 g H2SO4. 0.250 g H2SO4 x 1 mole x 1 L = 0.0102 L 98.12 g 0.250 mole 5. 1.50 g of NaCl is dissolved in 100.0 mL of water. Calculate the concentration. 6.
1. 25 cm3 of a solution of 0.1 moldm-3 NaOH reacts with 50 cm3 of a solution of hydrochloric acid. What is the molarity of the acid? 2. 25.0 cm3 of a 0.10 moldm-3 solution of sodium hydroxide was titrated against a solution of hydrochloric acid of unknown concentration.
A gas occupies 300.0 mL at 20.0° C. What would be its volume at 0° C, if the pressure is constant? 4. What is the mass of 2.00 L of ethane, C2H6, at STP? 5. A 0.500 g sample of boron hydride, B4H10, burns completely in excess oxygen.
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?
(2 points) Mg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq) 2. Determine the partial pressure of the hydrogen gas collected in the gas collection tube. (3 points) partial pressure H2 = total pressure - vapor pressure of water = 746mmHg - 19.8mmHg = 726mmHg 3. Calculate the moles of hydrogen gas collected. (4 points) n = 125 4.
3. Dilute acid solution: Use 0.01–0.1 M hydrochloric acid. 4. Sodium hydroxide solution: Use 0.01 M sodium hydroxide, 0.40 g/L. 5.
E) Water is a compound. 5. Which of the following are chemical processes? 1. rusting of a nail 2. freezing of water 3. decomposition of water into hydrogen and oxygen gases 4. compression of oxygen gas A) 1, 3, 4 B) 2, 3, 4 C) 1, 4 D) 1, 2 E) 1, 3 6. Which one of the following is the highest temperature?
(0.125)(0.1) = 0.0125 moles of solute b. Pour 50 mL of the stock solution to get the number of moles needed. 6. Exercise 6: a. (0.02) (1) = x/ 372.24 x=7.4 grams of sodium EDTA that is weighted out. b.
Conclusion 10 Grams of Potassium chlorate when decomposed produces 3.915576 grams oxygen gas and 6.083363 grams potassium chloride Atomic Weight of Magnesium Introduction In this lab we will determine the atomic weight of magnesium by measuring the amount of hydrogen gas evolved when hydrochloric acid reacts with magnesium. The reaction is as follows: Mg + 2HCl -> H2 + Mg2+ (aq) + 2Cl- (aq) There is a one to one relationship between the number of moles of hydrogen gas evolved and the
How many moles of gas does it take to fill a 1.0 L flask at a pressure of 1.5 atm at 100 celsius? (.049 mol) 2. What is the atmospheric pressure if the partial pressures of nitrogen, oxygen and argon are 604.5 mm Hg, 162.8 mm and .5 mm respectively? (767.8 mm Hg) 3. Describe the