Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- Sodium hypochlorite is the active ingredient in most household bleach products. One method of preparing this compound is as follows: Cl2(g) + 2N2OH(aq) → NaOCI (aq) + NaCl(aq) + H2O(1) In a certain experiment, 50.0 g chlorine was reacted with 50.0 g sodium hydroxide to yield 37.8 g sodium hypochlorite. (a) Calculate the theoretical yield (b) Calculate the percent yield.arrow_forwardBarium hydride reacts with water to produce barium hydroxide and hydrogen gas. BaH₂ (s) + 2 H₂O(1)→ Ba(OH)2 (aq) + H₂(g) If 6.389 g BaH2 is combined with 64.000 g H₂O, the reaction proceeds until all the BaH₂ is consumed. The hydrogen gas escapes to the environment, and the final weight of the flask is 70.204 g. The remaining water is evaporated, leaving 7.856 g Ba(OH)2. What mass of water is consumed in the reaction? g H₂O BO esc :0 F1 2 1086 TeTWE F2 # OCT 3 3 80 F3 $ 4 F4 R 65 % F5 T COMING MacBook Pro < 6 F6 Y & A 7 aa F7 * 00 U 8 DII F8 tv A S I F9 2 S F10 0 0 Save and Exit a F11arrow_forwardFor the following reaction, 21.9 grams of iron are allowed to react with 5.22 grams of oxygen gas. iron (s) + oxygen (g) →iron(II) oxide (s) What is the maximum amount of iron(II) oxide that can be formed? What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams gramsarrow_forward
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