Consider dilutions: M1V1 = M2V2, lets say M1 = 12.0 M and V2 = 1.OLand M2 = 2.0 M, would V2 be higher, lower or same (unchanged) O V2 must decrease in order to account for M2 being lower O V2 does not change O V2 must increase in order to account for M2 being lower

Given the following equations H/M=K LIN=KP Combine the two equations and solve for P

8-7. Suppose a 185 gram sample of hydrogen reacts with an excess of nitrogen dioxide as follows: 2 NO2 (g) + 7 H2 (g) → 2 NH3 (g) + 4 H2O(g) Both products are collected together (separate from any remaining reactants) in a 325 liter vessel at 512 K. a. How many moles of ammonia gas are produced? b. How many moles of water vapor are produced? c. What is the total pressure in the product collection vessel after the reaction is complete?  8-8. Suppose 93.4 grams of aluminum sulfide are added to 5.00 liters of a 0.844 M hydrochloric acid solution and the following reaction takes place: 6 HCl (aq) + Al2S3 (s) → 3 H2S (g) + 2 AlCl3 (aq) a. Which reactant is the limiting reactant? b. Briefly explain how you know which reactant is limiting. Be specific. Use complete sentences. c. What volume of hydrogen sulfide gas is collected at STP? d. How many grams of aluminum sulfide will be left over at the end? e. What is the final molarity of HCl?

c. Calculate the mole fraction of chlorine and its partial pressure in the mixture of gases produced. d. The van der Waals equation applies strictly to pure real gases.P = (nRT/ V-nb) – a(n2/V2) Suppose the gas mixture generated in the decomposition has the following parameters: a= 4.00 atm*L2/mol2 and b = 0.0330 L/mol. Determine the pressure of the gas mixture in part (b) using the van der Waals equation. Why is the result smaller than that in part (b)?

Hot gaes Expanding A mixture hot gases expands, changing volume from 2.45 L to 6.82 L, against a constant pressure of 3.22 atm. The P-Vwork involved is Latm .

Please answer the question Below.

a. Given the following set of values for a gas, calculate the unknown quantity: P = 743.3 mm Hg V = ? L n = = 0.1021 mol T = 23.3 °C V = L b. Given the following set of values for a gas, calculate the unknown quantity: P = ? atm V = 28.4 mL n = 0.007052 mol T = 20.5 °C P = c. Given the following set of values for a gas, calculate the unknown quantity: P= 1.079 atm T = atm V = 44.7 mL n = 0.003411 mol T = ? K K

What is the Qc for the following reaction, if a mixture contains gases with the following concentrations: CH4, 26 M; H2O, 24 M; CO, 26 M; H2 15 M, at a temperature of 760 0C? CH4(g) + H2O(g) CO(g) + 3H2(g)

Consider the following samples of gas: sample composition pressure temperature A 2.0mol Xe (g) 1.7atm 228.°C B 2.0mol Xe (g) 1.4atm 258.°C C 2.0mol Xe (g) 1.6atm 280.°C sample composition pressure temperature D 1.5mol He (g) 1.5atm 41.°C E 1.5mol Ar (g) 2.4atm 41.°C F 1.5mol Ne (g) 1.2atm 41.°C Draw the set of graphs below that show the distributions of the speed of the atoms in each sample.

If V= 9.14L at 24 C, Find V= ? at 49 C if pressure and moles are constant