CO(g) + Cl₂(g) COCI(g) Into a sealed 1.50 L flask, chemist placed 3.00 x 10² mol of phosgene gas (COCI) and heated it to 800.0 K. After the system reached equilibrium, the pressure of CO was found to be 0.504 bar. Calculate the equilibrium constant Kp for this reaction. After the system reached equilibrium, the pressure of CO was found to be 0.504 bar. Determine the phosgene (COCI,) pressure at equilibrium. CO(g) + Cl₂(g) COCI₂(g) 1

3. By means of Lewis structures, represent bonding between the following pairs of elements (Your structures should show whether the bonding is essentially ionic or covalent): (2 pts each) (d) Cs and Cl (e) Li and 0 (f) Cl and I

Consider the chemical reaction that takes place between solid magnesium and oxygen gas. In the reaction, identify which element in what species is oxidized? A) O₂ B) Mg(s) C) O in MgO D) Mg in MgO

Give the noble gas shorthand notation (ex: [He] 2s2 2p1) for Br       Give the noble gas shorthand notation (ex: [He] 2s2 2p1) for Ca+2       Give the noble gas shorthand notation (ex: [He] 2s2 2p1) for Zn

Consider the balanced reaction 5 A + 7 B → 5 C + 9 D. If 6.157 grams of B (MW = 31.84) are consumed, how many moles of A (MW = 38.29) are also consumed?

You have a 11.5 mg sample of blood that contains various proteins. Hemoglobin is the only protein in the sample containing Fe. Hemoglobin contains 3.83% by mass of a compound called heme (C₃₄H₃₂FeN₄O₄, MW = 616.49 g/mol). You find that your 11.5 mg blood sample contains 34.9 micrograms of Fe. What is the mass percent of hemoglobin in your protein sample?   -don't prematureley round