Question 6 V.J pus Concept: Gaseous substances are frequently involved in chemical reactions. If the pressure,...
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he appropriate gas law to solve questions 1-6. Show work. (2 pts) A certain amount of a gas at a constant temperature has a pressure of 5.50 atm and a volume of 10.0 mL. If the volume is decreased to 125.0 mL, what is the resulting pressure of the gas? : 924 a4m 125 O P v (2 pts) If 0.722 L of a certain gas at...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g)+O2(g)↽−−⇀2NO2(g) 2 NO ( g ) + O 2 ( g ) ↽ − − ⇀ 2 NO 2 ( g ) the standard change in Gibbs free energy is Δ?°=−72.6 kJ/mol Δ G ° = − 72.6 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are ?NO=0.300 atm P NO...
Calculate the volume of the gas when the pressure of the gas is 2.00 atm at a temperature of 298 K. There are 110. mol of gas in the cylinder. The value for the universal gas constant R is 0.08206 L⋅atm/(mol⋅K) . Express your answer numerically to four significant figures.
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g)+O2(g)↽−−⇀2NO2(g) the standard change in Gibbs free energy is Δ?°=−72.6 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are ?NO=0.500 atm , ?O2=0.400 atm , and ?NO2=0.750 atm ?
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N (8) + 3H2(g) + 2NH3(g) the standard change in Gibbs free energy is AGⓇ = -72.6 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN, = 0.200 atm, PH, = 0.450 atm, and PNH, = 0.750 atm? AG= L kJ/mol AG= kJ/mol
QUESTION 12 What is the total pressure exerted by a gaseous mixture that consists of 8.00g of methane and 12.00 g of ethane, C2H6, in a 3.50 L container maintained at 35.20 °C? O 0.400 atm O 0.741 atm O 3.13 atm O 6.49 atm O 16.5 atm
A sample of gaseous PCs was introduced into an evacuated flask so that the pressure of pure PCI would be 0.48 atm at 433 K. However, PCIE decomposes to gaseous PCI; and Cly, and the actual pressure in the flask was found to be 0.80 atm. Calculate Ko for the decomposition reaction below at 433 K. PCI() = PCI;(9) + Cl2(0) Also calculate K at this temperature. At a particular temperature, 11.1 mol of SO3 is placed into a 3.8-L...
Homework week 6 1. How do gaseous, liquid, and solid methanol (CHO) compare in each of the following features: (a) density; (b) the space between the molecules; (c) the attractive force between the molecules? 2. Convert each pressure unit to the indicated unit. a. 3.0 atm to mm Hg b. 720 mm Hg to psi c. 424 mm Hg to atm 3. A sample of nitrogen gas has a volume of 15.0 mL at a pressure of 0.50 atm. What...
Class-work ch.6 and ch. 10 Name 1) What is the final pressure (expressed in atm) of a 3.05 L system initially at 7wHg and 2 that is compressed to a final volume of 2.51 L at 273 K 1) 2) What is the pressure of a 1.0 L flask containing 0.60g of He at 25°C? (R-0.0821 L atm/mol K) 3) What is the volume of 28.0 g of nitrogen gas at STP? 3) 4) What is the final pressure of...
5. The equilibrium constant, KcKc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, KpKp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)Δn where R=0.08206 L⋅atm/(K⋅mol)R=0.08206 L⋅atm/(K⋅mol), TT is the absolute temperature, and ΔnΔn is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)⇌2NH3(g) for which Δn=2−(1+3)=−2 For the reaction 3A(g)+2B(g)⇌C(g) KcKc...