Enter your answer in the provided box. How many liters of gaseous hydrogen bromide at 31°C...
How many liters of gaseous hydrogen bromide at 69°C and 0.889 atm will a chemist need if she wishes to prepare 3.50 L of 1.20 M hydrobromic acid
How many liters of gaseous hydrogen bromide at 36°C and 0.898 atm will a chemist need if she wishes to prepare 3.50 L of 1.20 M hydrobromic acid?
How many liters of gaseous hydrogen bromide at 12°C and 0.959 atm will a chemist need if she wishes to prepare 3.50 L of 1.20 M hydrobromic acid?
Enter your answer in the provided box. If you want to prepare 0.50 liters of a 0.25 M solution of NaNO3, how many grams of the salt should you weigh out?
Enter your answer in the provided box. How many moles of solute particles are present in 1 L (exact) of aqueous 1.15 M KBr? □mol of particles
Enter your answer in the provided box. Ammonium hydrogen sulfide decomposes according to the following reaction, for which Kp = 0.11 at 250°C: NH4HS(S) = H2S(g) + NH3(g) If 53.1 g of NH4HS() is placed in a sealed 5.0-L container, what is the partial pressure of NH3(g) at equilibrium? Рун, = atm
Enter your answer in the provided box. Roasting galena [lead(II) sulfide) is an early step in the industrial isolation of lead. How many liters of sulfur dioxide, measured at STP, are produced by the reaction of 5.75 kg of galena with 193 L of oxygen gas at 220°C and 2.00 atm? Lead(II) oxide also forms. LSO2
Enter your answer in the provided box. Ammonium hydrogen sulfide decomposes according to the following reaction, for which Kp =0.11 at 250°C NH HS(s) H2S() +NH3() If 60.5 g of NH HS(s) is placed in a sealed 5.0-L container, what is the partial pressure of NH3(g) at equilibrium? PN atm Enter your answer in the provided box. Even at high temperatures, the formation of NO is not favored: (K-4.10x 10 at 2000°C) N28)+O2(g)= 2 NO(g) What is (NO] when a...
Enter your answer in the provided box. Describe how to prepare 0.350 L of 0.650 M HCI solution, starting with a 2.00 M HCI solution. What volume (in L) of the 2.00 M solution will you need?
Enter your answer in the provided box. Calculate the volume of 11.7 M sulfuric acid that must be added to water to prepare 5.879 L of a 0.808 M solution.