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Nat2105 [25]
3 years ago
15

PLEASE HELP ME ASAP PLEASE!!!

Chemistry
1 answer:
Sliva [168]3 years ago
4 0

Answer:

\large \boxed{\text{1763 psi}}

Explanation:

We can use Dalton's Law of Partial Pressures:

Each gas in a mixture of gases equals its pressure independently of the other gases

\begin{array}{rcl}p_{\text{NO2}} + p_{\text{CO2}} & = & p_{\text{tot}} \\p_{\text{NO2}} + \text{795 psi} & = &\text{2558 psi}  \\p_{\text{NO2}} & = &\text{2558 psi - 795 psi} \\& = & \textbf{1763 psi}\\\end{array}\\\text{The partial pressure of nitrogen dioxide is $\large \boxed{\textbf{1763 psi}}$}

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2 years ago
Which atom would be expected to have a half-filled 6s subshell
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Explanation:

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3 years ago
Colligative property definition chemistry
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3 years ago
Enter the ionic equation, including phases, for the reaction of AgNO3(aq) with K2SO4(aq).
gogolik [260]
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3 0
3 years ago
In the decomposition potassium nitride, 10.65 g of nitrogen form. How much potassium nitride was present initially ?
leonid [27]

Answer:

Mass =  99.8 g  

Explanation:

Given data:

Mass of potassium nitride = ?

Mass of nitrogen produced = 10.65 g

Solution:

Chemical equation:

2K₃N→ 6K + N₂

Moles of nitrogen:

Number of moles = mass/ molar mass

Number of moles =  10.65 g / 28 g/mol

Number of moles = 0.38 mol

Now we will compare the moles of nitrogen with potassium nitride.

                        N₂              ;         K₃N

                         1               :            2

                         0.38          :          2×0.38 =0.76

Mass of potassium nitride:

Mass = molar mass × number of moles

Mass =    131.3 g/mol ×   0.76 mol

Mass =  99.8 g    

7 0
3 years ago
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