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Olenka [21]
3 years ago
14

How many of these substances are elements?

Chemistry
1 answer:
aniked [119]3 years ago
8 0
There are three elements
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A gas mixture contains 3.00 atm of H2 and 1.00 atm of O2 in a 1.00 L vessel at 400K. If the mixture burns to form water while th
sleet_krkn [62]

Answer:

p_{H_2O}=2.00atm

Explanation:

Hello!

In this case, according to the following chemical reaction:

2H_2+O_2\rightarrow 2H_2O

It means that we need to compute the moles of hydrogen and oxygen that are reacting, via the ideal gas equation as we know the volume, pressure and temperature:

n_{H_2}=\frac{3.00atm*1.00L}{0.08206\frac{atm*L}{mol*K}*400K}=0.0914molH_2 \\\\n_{O_2}=\frac{1.00atm*1.00L}{0.08206\frac{atm*L}{mol*K}*400K}=0.0305molH_2

Thus, the yielded moles of water are computed by firstly identifying the limiting reactant:

n_{H_2O}^{by\ H_2} = 0.0914molH_2*\frac{2molH_2O}{2molH_2} =0.0914molH_2O\\\\n_{H_2O}^{by\ O_2} = 0.0305molO_2*\frac{2molH_2O}{1molO_2} =0.0609molH_2O

Thus, the fewest moles of water are 0.0609 mol so the limiting reactant is oxygen; in such a way, by using the ideal gas equation once again, we compute the pressure of water:

p_{H_2O}=\frac{0.0609molH_2O*0.08206\frac{atm*L}{mol*K}*400K}{1.00L}\\\\ p_{H_2O}=2.00atm

Best regards!

7 0
3 years ago
The calorimeter pictured below shows the final temperature after calcium chloride was added to water. (The initial temperature w
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It’s probably D or c
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What is the process that changes one set of chemicals into another set of chemicals? A. cohesion B. hydrogen bonding C. chemical
diamong [38]
I think the correct answer from the choices listed above is option C. Chemical reaction is the process <span>that changes one set of chemicals into another set of chemicals. In a chemical reaction, old bonds are broken down forming new bonds therefore new </span>substances<span> with new properties.</span>
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3 years ago
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Which of the following is a homogeneous mixture? a. Na(s) b. H2O(l) c. Cl2(g) d. NaCl(aq)
iVinArrow [24]

Answer:

H²0 is answer is H20 ok please

7 0
3 years ago
A sample of He gas (3.0 L) at 5.6 atm and 25°C was combined with 4.5 L of Ne gas at 3.6 atm and 25°C at constant temperature in
In-s [12.5K]

Answer:

3.6667

Explanation:

<u>For helium gas:</u>

Using Boyle's law  

{P_1}\times {V_1}={P_2}\times {V_2}

Given ,  

V₁ = 3.0 L

V₂ = 9.0 L

P₁ = 5.6 atm

P₂ = ?

Using above equation as:

{P_1}\times {V_1}={P_2}\times {V_2}

{5.6}\times {3.0}={P_2}\times {9.0} atm

{P_2}=\frac {{5.6}\times {3.0}}{9.0} atm

{P_1}=1.8667\ atm

<u>The pressure exerted by the helium gas in 9.0 L flask is 1.8667 atm</u>

<u>For Neon gas:</u>

Using Boyle's law  

{P_1}\times {V_1}={P_2}\times {V_2}

Given ,  

V₁ = 4.5 L

V₂ = 9.0 L

P₁ = 3.6 atm

P₂ = ?

Using above equation as:

{P_1}\times {V_1}={P_2}\times {V_2}

{3.6}\times {4.5}={P_2}\times {9.0} atm

{P_2}=\frac {{3.6}\times {4.5}}{9.0} atm

{P_1}=1.8\ atm

<u>The pressure exerted by the neon gas in 9.0 L flask is 1.8 atm</u>

<u>Thus total pressure = 1.8667 + 1.8 atm = 3.6667 atm.</u>

6 0
3 years ago
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