<h3>Answer:</h3>
Mass = 96.47 g
<h3>
Solution:</h3>
Data Given:
M.Mass = 28.97 g.mol⁻¹
Moles = 3.33 mol
Mass = ??
Formula Used:
Moles = Mass ÷ M.Mass
Solving for Mass,
Mass = Moles × M.Mass
Putting values,
Mass = 3.33 mol × 28.97 g.mol⁻¹
Mass = 96.4701 g
Rounding to four significant numbers,
Mass = 96.47 g
Answer:
59.2 grams
Explanation:
We are given that 70.4% of the weight of the total 200 g of the concentration is made up of nitric acid, the remaining information is not required to solve the problem. Since water and nitric acid are the only components of the solution, the total weight of water is given by:
There are 59.2 grams of water in this solution.
Answer:
ΔH=15000
J = 15KJ
Explanation:
In this exercise you have find the enthalpy of reaction this is the difference between enthalpy of reactans and products,
For the following equation
H2A(aq) + 2 BOH(aq) → B2A(aq) + 2 H2O(l)
We know that 0.20 moles of BOH reacted with excess amount of H2A solution and 1500. J
so,
(2mol/0,2mol)*1500J=15000J
for de reactions exothermics tha enthalpy is negative so:
ΔH=15000
J = 15KJ
The answer is A, i'm also on study island on this test. It has a star next to it. So yep we're right!
You would use a pie chart to best display your results
