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Determine the number of bonding electrons and the number of nonbonding electrons in the structure of CS2
Calculate the heat given off by the burning Mg in kJ/g. b)Calculate the heat given off by burning Mg in kJ/mol
Zn(s) + 2AgNO3(aq) --> 2Ag(s) + Zn(NO3)2(aq) When 216 g of silver was produced, determine the mole(s) of silver nitrate would be required.
Determine delta H of this reaction (kJ/mol H 2 SO 4 ) - When 24.4 mL of 0.500M sulphuric acid ,H 2 SO 4 is combined to 24.4ml of 1.00M potassium hydroxide KOH in a coffee cup calorimeter
Identify each of the following unbalanced aqueous reactions as an acid/base reaction (a), a redox reaction (r) or a precipitation reaction (p).
Calculate the pH of a solution that is 0.253M in nitrous acid (HNO_2) and 0.111M in potassium nitrite (KNO_2). Acid dissociation constant
Suppose that a student performing this experiment recorded the concentration of NaOH solution as 0.513 M, instead of the correct value of 0.531 M.
Suppose some of the solid Calcium Hydroxide is inadvertently transferred along with a supernatant liquid for analysis. Will more, less, or the same amount of HCL titrant be used for analysis
Rubidium has two naturally occuring isotopes. The relative abundance of rubidium-85 is 72.17%; its atomic mass is 86.91 amu. Determine the average atomic mass of rubidium.
Calculate the mass percent of a solution that is prepared by adding 61.4 g of rm NaOH to 413 g of {rm H_2O}.
Explain how it is that the concentrations of chloride ions in these beakers are different even though the concentrations of each substance(compound) are the same.
What is the name of the compound (NH4)3PO3? Why is special about this compound? Choose one answer. a. Ammonium phosphate; this covalent compound is made up of two polyatomic ions, ammonium and phosphate.
In a controlled greenhouse at 30.0C and 1.0 atm a crop of seeding tomato plants was found to consume 380 L of carbon dioxide gas during photosynthesis. Assuming 100% yield what a mass of glucose was produced for the growing plants?
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