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2 years ago

How many moles of C2H2 are needed to react completely with 84.0 mol O2?

Chemistry

2 answers:

docker41 [41]2 years ago

5 0

Answer: 33.6 moles

Explanation:

According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

Combustion of ethylene is represented by following balanced equation:

$2C_2H_2+5O_2\rightarrow 4CO_2+2H_2O$

According to stoichiometry:

5 moles of $O_2$ react completely with = 2 moles of $C_2H_2$

Thus 84.0 moles of $O_2$ react completely with = $\frac{2}{5}\times 84.0=33.6$ moles of $C_2H_2$

Thus 33.6 moles of $C_2H_2$ are needed to react completely with 84.0 mol $O_2$

Airida [17]2 years ago

3 0

33.6 moles are needed to completely react with 84.0 moles of O2

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The pressure in an automobile tire is 2.0 atm at 27°C. At the end of a journey on a hot summer day the pressure has risen to 2.2

Kruka [31]

Hey there!

For this we can use the combined gas law:

$\frac{P_{1}V_{1} }{T_{1}} = \frac{P_{2}V_{2} }{T_{2}}$

We are only working with pressure and temperature so we can remove volume.

$\frac{P_{1} }{T_{1}} = \frac{P_{2} }{T_{2}}$

P₁ = 2 atm

T₁ = 27 C

P₂ = 2.2 atm

Plug these values in:

$\frac{2atm}{27C} = \frac{2.2atm}{T_{2}}$

Solve for T₂.

$2atm = \frac{2.2atm}{T_{2}}*27C$

$2atm * T_{2}={2.2atm}*27C$

$T_{2}={2.2atm}\div2atm*27C$

$T_{2}=1.1*27C$

$T_{2}=29.7C$

Convert this to kelvin and get 302.85 K, which is closest to B. 330 K.

Hope this helps!

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2 years ago

One gram of salt in swimming pool of water could be considered a _____ solution.

omeli [17]

Answer:

Soluable

Explanation:

Because salt dissolves in water.. Your question has no background information to go off of

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2 years ago

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Which of the following is the correctly balanced chemical equation for the reaction of Ca(OH)2 and HNO3?

Bad White [126]

Ca(OH)2+HNO3———> Ca(NO3)2+H2O

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3 years ago

6. If 0.500 mol NaN3 react, what mass in grams of nitrogen will result?

lions [1.4K]

Answer:

21 g of N₂ are produced by the decomposition

Explanation:

The reaction is: 2 NaN3 → 2 Na + 3 N2

2 moles of sodium nitride decompose in order to produce 2 moles of Na and 3 moles of nitrogen gas.

According to stoichiometry, ratio is 2:3. Therefore we say,

2 moles of nitride can produce 3 moles of N₂

Then, 0.5 moles of NaN₃ will produce (0.5 . 3) / 2 = 0.75 moles of N₂

We convert the moles to mass, to find the answer

0.75 mol . 28 g / 1 mol = 21 g

7 0

2 years ago

Determine the [H3O+] in a 0.265 M HClO solution. The Ka of HClO is 2.9 × 10-8.

dexar [7]

8.8 × 10-5 M is the [H3O+] concentration in 0.265 M HClO solution.

Explanation:

HClO is a weak acid and does not completely dissociate in water as ions.

the equation of dissociation can be written and ice table to be formed.

HClO +H2O ⇒ ClO- + H3O+

I 0.265 0 0

C -x +x +x

E 0.265-x +x +x

Now applying the equation of Ka, where Ka is given as 2.9 × 10-8.

Ka = $\frac{[ClO-][H3O+]}{[HClO]}$

2.9 × 10^-8 = $\frac{[x] [x]}{[0.265-x]}$

$x^{2}$ = 7.698 x $10^{-9}$

x = 8.8 × 10-5 M

The hydronium ion concentration is 8.8 × 10-5 M in 0.265 M solution of HClO.

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2 years ago