Download the following file to begin.  e_Landscape_Sales.xlsx When finished, upload only the Landscape and Garden sales worksheet for this question. Question 3: Landscape and Garden Sales (Excel) Start Excel and open the file e_Landscape_Sales. Save the document as Lastname_Firstname_Exam_Landscape_Sales using your first and last name. Change the theme to Basis. Group the two worksheets. Merge and center the title across the range A1:G1 and apply the Title style. Merge and center the subtitle across the range A2:G2 and apply the Heading 1 style. Apply the Heading 4 style to cells B11:G11. Insert a formula to calculate the Product Total in cells E12:E16 for each of the products. Insert a formula to calculate the monthly total for each of the months in cells B17:E17. Calculate the percent of the total in cells F12:F16 using an absolute reference, and apply Percent Style with no decimal places and center the values within the cells. Change the width of columns B:E to 14.5. Apply the Accounting Number Format with zero decimal places to cells B12:E12 and B17:E17. Apply the Total style to cells B17:E17. For the range B13:E16, apply the Comma Style with zero decimal places. In cells B4:B7, enter formulas to calculate the Average, Median, Min, and Max for the Product Total in cells E12:E16. Apply the Accounting Number Format. In cells G12:G16, enter a formula that displays “Yes” if the Percent of Total is less than or equal to 10% (use

A 1.00 L solution saturated at 25 °C with calcium oxalate (CaC2O4) contains 0.0061 g of CaC2O4. Calculate the Ksp for this salt at 25 °C.

Calculate the change in Gibbs free energy, ΔG, for the following reaction, H2(g) + Zn2+(aq) → Zn(s) + 2 H+(aq), where the standard reduction potential for the reduction of Zn2+ to Zn(s) is -0.76 V. Given the Faraday constant is 96,485 J/V-mol.

Predict whether the equivalence point for a titration of NH3 with HCl will be above, below, or at pH 7.0.

Given the standard reduction potentials for the following half reactions. Determine which combination of these half-cell reactions leads to the cell reaction with the largest positive cell potential. Ag+(aq) + e- → Ag(s) 0.80V Cu2+(aq) + 2e- → Cu(s) 0.34V Ni2+(aq) + 2e- → Ni(s) -0.28 V Cr3+(aq) + 3e- → Cr(s) -0.41 V

Consider the reaction, B(aq) + H2O(l) → BH+(aq) + OH-(aq). If the salt of BH+(aq) is added, how is the equilibrium constant affected?

The first-order decomposition of N2O5 was studied at a particular temperature and found to have a rate constant of 6.2 x 10-4s-1. What is the half-life for the decomposition under these conditions?

A buffer is made by adding 0.300 mol CH3COOH and 0.300 mol CH3COONa to enough water to make 1.000 L of solution. The pH of the buffer is 4.74. Calculate the pH of this solution after 15.0 mL of 4.0 M NaOH(aq) solution is added.

If the equilibrium concentration (also known as the molar solubility) of CaF2 is 1.24 x 10-3M at 35 °C, what is Ksp at this temperature?

Which would be correct expression of the solubility product constant, Ksp, for Fe(OH)3?