The sulfate ion, SO4 2-, can be drawn in many ways. If youminimize formal charge on the sulfur, how many S=O double bonds should you draw in the Lewis structure?(a) 0 (b) 1 (c) 2 (d) 3 (e) 4

Hint: if the ratio of moles of H2O to moles of anhydrous KAl(SO4)2 was 4, then the empirical formula would be: KAl(SO4)2•4H2O. Write the empirical formula for the hydrated KAl(SO4)2, based on moles of anhydrous KSI(SO4)2= 0.046 mol molar mass of H2O= 18g/ mol moles of H2O= 0.0444mol ratio pf moles H20 to moles of anhydrous KAI(SO4)2= 9.65/1 .

Calculate a) the molar concentration of Na+ and SO4^2- given that the average density of seawater is 1.02 g/mL. b) the pNa and pSO4 for the seawater Seawater contains an average of 1.08 x 10^3 ppm of Na+ and 270ppm of SO4^2- .

Step 2: Find the molar mass of KAl(SO4)2 and show work here; Step 3: Find the moles with work shown: grams of the dry salt divided by the molar mass = moles; B. Calculate the ratio of moles of H 2 O to moles of anhydrous KAl(SO 4) 2. Note: Report the ratio to the closest whole number.

Turn off browse mode or quick nav, Tab to items, Space or Enter to pick up, Tab to move, Space or Enter to drop. grams O2 grams Fe2O3grams O2 grams Fe2O3 moles FeFe moles O2O2 Answer Bank grams FeFe grams O2O2 grams Fe2O3Fe2O3 moles Fe2O3Fe2O3 Step 2: Show the conversions required to solve this problem and calculate the grams of Fe2O3Fe2O3.

Calculate the ratio of moles of H2O to moles of anhydrous KAl(SO4)2. Show all work to answer this question by uploading an image of your calculations into Photo 3. Note: Report the ratio to the closest whole number. Write the empirical formula for the hydrated KAl(SO4)2, based on your experimental results and answer to Question 2.

Solution for Write the balanced chemical equation for conversion of Al(s) to KAl(SO4)2·12H2O(s) in aqueous solution.

Q: Write the balanced chemical equation for conversion of Al(s) to KAl(SO4)2·12H2O(s) in aqueous… A: The balanced equation is the equation in which the number of atoms of each elements are equal at…

Write the empirical formula for the hydrated KAl(SO4)2, based on your experimental results and answer to Question 2 (the answer was 65). Show all work including units. Hint: if the ratio of moles of H2O to moles of anhydrous KAl(SO4)2 was 4, then the empirical formula would be: KAl(SO4)2•4H2O.

For the chemical reaction, Fe2O3 + 3 SO3 à Fe2(SO4)3, calculate the number of moles of SO3 you will need to completely react with 6.45 moles of Fe2O3. Select the closest value. arrow_forward