Sent a pic that shows the work and answer is in box.
Complete Question:
A chemist adds 55.0 mL of a 1.1M barium acetate (Ba(C2H3O2)2) solution to a reaction flask. Calculate the mass in grams of barium acetate the chemist has added to the flask. Round your answer to 2 significant digits.
Answer:
15 g
Explanation:
The concentration of the barium acetate is given in mol/L (M), thus, the number of moles (n) of it is the concentrantion multiplied by the volume (55.0 mL = 0.055 L):
n = 1.1 * 0.055
n = 0.0605 mol
The molar mass of the substance can be calculated by the sum of the molar mass of each element, which can be found at the periodic table. Thus:
Ba = 137.33 g/mol
C = 12.00 g/mol
H = 1.00 g/mol
O = 16.00 g/mol
Ba(C2H3O2)2 = 137.33 + 4*12 + 6*1 + 4*16 = 255.33 g/mol
The molar mass is the mass divided by the number of moles, thus the mass (m) is the molar mass multiplied by the number of moles.
m = 255.33 * 0.0605
m = 15.45 g
Rounded by 2 significant digits, m = 15 g.
Explanation:
try to arrange using the given molecular formula
Explanation:
Oxygen and Nitrogen. is the correct pair.
Answer:
1. right 2. left 3. left 4. left 5. left
Explanation:
1. N2 is a reactant, so adding more will push the reaction away from N2 which will be right, towards the products
2. treat heat as a product, so by increasing temp you increase heat and you push the reaction away from heat which will be left, towards the reactants
3. Adding NH3 will push the reaction away from it, so it'll move left, towards reactants
4. When you decrease pressure, the reaction will move to the side with more moles, since the left side has 4 moles and the right only has 2, it'll move left
5. by removing H2, the equillibrium will shift left in order to restore balance.