Question

Gas stoichiometry 1. Assume that 5.60 L of hydrogen gas at STP reacts with copper (II)oxide according to the following balanced equation: CuO (s) + H2(g) → Cu (s) + H20 (9) a. How many moles of H2 react? b. How many moles of copper are produced? c. How many grams of copper are produced? Partial pressure: 1. What is the total pressure exerted by a mixture of 2.00 g of H2(g) and 8.00 g of N2(g) at 273 K in a 10.0-L vessel? Relating Mole Fractions and Partial Pressures 1. A study of the effects of certain gases on plant growth requires a synthetic atmosphere composed of 1.5 mol percent CO2, 18.0 mol percent O2, and 80.5 mol percent Ar. (a) Calculate the partial pressure of Oz in the mixture if the total pressure of the atmosphere is to be 745 mmHg. (b) If this atmosphere is to be held in a 121-L space at 295 K, how many moles of o, are needed? Partial pressure and reaction 1. When a sample of KCIO, is partially decomposed in the setup shown in the picture, the volume of gas collected is 0.250 L at 26 °C and 765 mmHg total pressure.

Answer 1

5875 * 0-08 2x 273 3 atm. 1) 22:46 H and he a) 0.25 moder of H₂ reacts. 5.6L H₂ (56 -0.25 md. Hy by 0-25 moles of Cu is produced 070-25*635)=1548754 is produced, PV=nRT: P-|(3)+44)]* 0-0822233 3-s18 atomi 1800/PL- PL 108,75= 1854-min Hg 1 = 10-176 afin ] by mi to 01726 1324 = [0*88 medan pod in required. a) na Pr (7)*0.25 -001 moles. If by KCOQ = KCl +O2. Thing/O-01 modes -= 1-225 gmsel decomposed 100 12 @moto required - RT 0082x295 RT 00082x299 were collected. Amount:(0-01x12255 * Koo were