1-Calculate the volume in liters of a ×2.710−6M mercury(II) iodide solution that contains 900.mg of mercury(II) iodide HgI2
. Round your answer to 2 significant digits.
2-Suppose a 500.mL flask is filled with 1.7mol of Cl2 and 1.6mol of HCl. The following reaction becomes possible:
H2g+Cl2g 2HClg
The equilibrium constant Kfor this reaction is 9.55 at the temperature of the flask.Calculate the equilibrium molarity of
HCl Round your answer to two decimal places.
1-Calculate the volume in liters of a ×2.710−6M mercury(II) iodide solution that contains 900.mg of mercury(II)...
Calculate the volume in liters of a ×2.2710−6M mercury(I) chloride solution that contains 900.mg of mercury(I) chloride Hg2Cl2. Round your answer to 3 significant digits.
A chemist prepares a solution of mercury(II) iodide (HgI2) by measuring out 5.9mg of mercury(II) iodide into a 350.mL volumetric flask and filling the flask to the mark with water.Calculate the concentration in mol/Lof the chemist's mercury(II) iodide solution. Be sure your answer has the correct number of significant digits.
A chemist prepares a solution of mercury(II) iodide (HgI,) by measuring out 2.2 mg of mercury(II) iodide into a 500. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's mercury(II) iodide solution. Be sure your answer has the correct number of significant digits. mol/L X 5 ?
Suppose a 500.mL flask is filled with 0.50mol of H2 and 0.70mol of HCl. The following reaction becomes possible: H2g+Cl2g -> 2HClg The equilibrium constant K for this reaction is 1.17 at the temperature of the flask. Calculate the equilibrium molarity of H2. Round your answer to two decimal places.
= STOICHIOMETRY Calculating molarity using solute moles calculating A chemist prepares a solution of mercury(IT) iodide (Hgl) by measuring out 0.00253 umol of mercury(II) iodide into a 300 mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in moll of the chemist's mercury(II) iodide solution. Round your answer to 3 significant digits. 2
A chemist adds 405.0 mL of a 5.1 * 10 mM mercury(II) iodide (Hg12) solution to a reaction flask. Calculate the micromoles of mercury(II) iodide the chemist has added to the flask. Be sure your answer has the correct number of significant digits. Πμ mol x I ?
A chemist adds 150.0 ml. of a 5.5 x 10 mmol/L mercury(II) iodide (Hgl) solution to a reaction flask. Calculate the mass in micrograms of mercury(II) todide the chemist has added to the flask. Round your answer to 2 significant digits 0.9 X 5 ?
Suppose a 500. mL flask is filled with 1.9 mol of Cl2, 0.70 mol of HCl and 1.7 mol of CCI4. The following reaction becomes possible Cl2(g)+ CHCI3)HCI (g)+CCI4g) The equilibrium constant K for this reaction is 7.09 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places
Suppose a 500.mL flask is filled with 0.10mol of Cl2, 0.40mol of HCl and 0.80mol of CCl4. The following reaction becomes possible: +Cl2gCHCl3g +HClgCCl4g The equilibrium constant K for this reaction is 0.116 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places.
Suppose a 250. mL. flask is filled with 1.8 mol of Cl2 and 0.60 mol of HCl. The following reaction becomes possible: H(+Cl()2HCI) The equilibrium constant K for this reaction is 8.25 at the temperature of the flask. Calculate the equilibrium molarity of Cl2. Round your answer to two decimal places.