Explanation:
Since pressure remained constant, we can eliminate P from the equation
Doing some algebra and converting temperature to Kevin by adding 273, you should obtain the same result.
You go fishing and obtain some less weights for your trip. Lead’s density is 11.34 g/mL. If there are 50 weights in a 250 mL box
1 answer:
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Answer is in picture below.
Use 100 grams of the compound:
ω(Cl) = 85.5% ÷ 100%.
ω(Cl) = 0.855; mass percentage of the chlorine in the compound.
m(Cl) = 0.855 · 100 g.
m(Cl) = 85.5 g; mass of chlorine.
m(C) = 100 g - 85.5 g.
m(C) = 14.5 g; mass of carbon.
n(Cl) = m(Cl) ÷ M(Cl).
n(Cl) = 85.5 g ÷ 35.45 g/mol.
n(Cl) = 2.41 mol; amount of chlorine.
n(C) = 14.5 g ÷ 12 g/mol.
n(C) = 1.21 mol; amount of carbon.
n(Cl) : n(C) = 2.41 mol : 1.21 mol = 2 : 1.
This compound is dichlorocarbene CCl₂.
This is an incomplete question, here is a complete question.
Hydrogen azide, HN₃, decomposes on heating by thefollowing unbalanced reaction:
If 3.0 atm of pure HN₃ (g) is decomposed initially,what is the final total pressure in the reaction container? Whatare the partial pressures of nitrogen and hydrogen gas? Assume thatthe volume and temperature of the reaction container are constant.
Answer : The partial pressure of and
gases are, 4.5 atm and 1.5 atm respectively.
Explanation :
The given unbalanced chemical reaction is:
This reaction is an unbalanced chemical reaction because in this reaction number of hydrogen and nitrogen atoms are not balanced on both side of the reaction.
In order to balance the chemical equation, the coefficient '2' put before the and the coefficient '3' put before the
then we get the balanced chemical equation.
The balanced chemical reaction will be,
As we are given:
The pressure of pure = 3.0 atm
From the reaction we conclude that:
Number of moles of = 3 mol
Number of moles of = 1 mol
Now we have to calculate the mole fraction of and
and,
Now we have to calculate the partial pressure of and
According to the Raoult's law,
where,
= partial pressure of gas
= total pressure of gas = 6.0 atm
= mole fraction of gas
and,
Thus, the partial pressure of and
gases are, 4.5 atm and 1.5 atm respectively.