With all the coefficient set to 1, how can you tell that the equation is not balanced?
1 answer:
Answer:
Well for any equation if all the coefficients are set to 1, this might result in unequal numbers of atoms of the same element on both sides
Explanation:
For example:
(for this equation all the coefficient (the number before element) are 1 but you can clearly see it is not balanced because one side has 1 A atom and other side has 2 B atoms....therefore we need to balance em.
Here both atoms are balanced.
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Answer:
a) 0,2% w/v
b) r=500
c) 0,0182 M
d) 0,0145 m
e) 0,0137 equivalents
Explanation:
a) % w/v means mass of solute in grams per 100 mililiter of solution. Thus:
%w/v= ×100 = 0,2%w/v
b) Ratio strength is a way to express concentration. For w/v is in 1g of solute <em>r</em> mililiters of solution have. Thus, r = 500 because we have in the first 1 g of CaCl₂ in 500 mL of solution.
c) Molarity is moles of solute per liter of solution, thus:
1,000 g of CaCl₂ × = 9,09×10⁻³ moles of CaCl₂
500 mL of solution × = 0,500 L of solution
M = = 0,0182 M
d) Molality is moles of solute per kg of solution.
Specific gravity is the ratio between density of the solution and density of a reference substance (Usually water). With a specific gravity of 0,8:
kg of solution = 0,500 L of solution × =<em> </em><em>0,625 kg of solution</em>
m = = 0,0145 m
e) In a salt, equivalents are the number of moles ables to replace one mole of charge. In CaCl₂ is ¹/₂ because with ¹/₂ moles of CaCl₂ it is possible to replace 1 mole of charges. Thus, in 1,5 L there are:
1,5 L × ×
= 0,0137 equivalents
I hope it helps!
Answer : The mass of the oxygen gas produced in grams and the pressure exerted by the gas against the container walls is, 96 grams and 1.78 atm respectively.
Explanation : Given,
Moles of = 2.0 moles
Molar mass of = 32 g/mole
Now we have to calculate the moles of
The balanced chemical reaction is,
From the balanced reaction we conclude that
As, 2 mole of react to give 3 mole of
So, 2.0 moles of react to give
moles of
Now we have to calculate the mass of
Therefore, the mass of oxygen gas produced is, 96 grams.
Now we have to determine the pressure exerted by the gas against the container walls.
Using ideal gas equation:
where,
P = pressure of oxygen gas = ?
V = volume of oxygen gas
T = temperature of oxygen gas =
R = gas constant = 0.0821 L.atm/mole.K
w = mass of oxygen gas
= density of oxygen gas = 1.429 g/L
M = molar mass of oxygen gas = 32 g/mole
Now put all the given values in the ideal gas equation, we get:
Thus, the pressure exerted by the gas against the container walls is, 1.78 atm.