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3 years ago

If I have 6 moles of a gas at a pressure of 3.4 atm and a volume of 10 liters, what

Chemistry

1 answer:

ch4aika [34]3 years ago

8 0

Answer:

The temperature is 69.05 K.

Explanation:

We have,

Number of moles are 6

Pressure is 3.4 atm and a volume of 10 liters.

It is required to find the temperature. It can be calculated using gas law equation. It says that,

$PV=nRT$

P is pressure

V is volume

n is number of moles

R is gas constant, $R=0.082057\ L-atm/mol-K$

T is temperature

Plugging all the values we get :

$T=\dfrac{PV}{nR}\\\\T=\dfrac{3.4\times 10}{6\times 0.082057}\\\\T=69.05\ K$

So, the temperature is 69.05 K.

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A student reacted NiS2 (MM = 122.83 g/mol) with O2 (MM=32.00 g/mol) to make SO2 (MM=64.07 g/mol) according to this balanced equa

Mice21 [21]

Answer:

Theoretical yield of SO₂ is 1.56 × 10² g

Explanation:

Given data:

Mass of NiS₂ = 1.50 ×10² g

Mass of O₂ = 2.420 ×10² g

Theoretical yield of SO₂ = ?

Solution:

Chemical equation:

2NiS₂ + 5O₂ → 2NiO + 4SO₂

Moles of NiS₂:

Number of moles = mass/ molar mass

Number of moles = 1.50 ×10² g / 122.83 g/mol

Number of moles = 1.22 mol

Moles of O₂:

Number of moles = mass/ molar mass

Number of moles = 2.420 ×10² g / 32 g/mol

Number of moles = 7.56 mol

Now we compare the moles of SO₂ with NiS₂ and O₂.

NiS₂ : SO₂

2 : 4

1.22 : 4/2×1.22 = 2.44

O₂ : SO₂

5 : 4

7.56 : 4/5×7.56 =6.05

Moles of SO₂ produced by NiS₂ are less it will limiting reactant.

Mass of SO₂ = moles × molar mass

Mass of SO₂ = 2.44 mol × 64.07 g/mol

Mass of SO₂ = 156.33 g

So theoretical yield of SO₂ is 1.56 × 10² g

4 0

3 years ago

A 10.00 g sample of a soluble barium salt is treated with an excess of sodium sulfate to precipitate 11.21 g BaSO4 (M- 233.4). W

aliina [53]

Answer:

The salt is barium chloride.

Explanation:

$BaX_2++Na_2SO_4\rightarrow BaSO_4+2NaX$

Moles of barium sulfate = $\frac{11.21 g}{233.38 g/mol}=0.0480 mol$

According to reaction, 1 mol of barium sulfate is produced from 1 mol of $BaX_2$ .

Then 0.0480 moles will be produced from:

$\frac{1}{1}\times 0.0480 mol=0.0480 mol$ of $BaX_2$ .

Mass of $BaX_2$ used = 10.00 g

Moles of $BaX_2$ =\frac{10.00 g}{\text{Molar mass}}[/tex]

$0.0480 mol=\frac{10.00}{\text{Molar mass}}$

Molar mass of $BaX_2$ = 208.33 g/mol

The nearest answer to our answer is $BaCl_2=208.2 g/mol$ .

The correct answer barium chloride with molar mass of 208.2 g/mol.

8 0

3 years ago

Consider the following reaction NHAHS(s)NH3(g) + H2S(g) If a flask maintained at 302 K contains 0.196 moles of NH4HS(s) in equil

quester [9]

Answer:

Kc = 3.72 × 10⁶

Explanation:

Let's consider the following reaction:

NH₄HS(g) ⇄ NH₃(g) + H₂S(g)

At equilibrium, we have the following concentrations:

[NH₄HS] = 0.196 M (assuming a 1 L flask)

[NH₃] = 9.56 × 10² M

[H₂S] = 7.62 × 10² M

We can replace this data in the Kc expression.

$Kc=\frac{[NH_{3}] \times [H_{2}S] }{[NH_{4}HS]} =\frac{9.56 \times 10^{2} \times 7.62 \times 10^{2}}{0.196} =3.72 \times 10^{6}$

7 0

3 years ago

C2H2 +<br> 02 --><br> CO2 +<br> H20

svlad2 [7]

Answer:

Explanation: This reaction is called a synthesis reaction. This is because a synthesis reaction is when two or more reactants combine/react together to form a single product. The two reactants carbon (C) and oxygen (O2) reacted together to form one single product: carbon dioxide (CO2)

5 0

2 years ago

What is the pH of a Koh solution that has [H+]=1.87×10^-13M

xenn [34]

PH=-log[H⁺]
pH=-log(1.87×10⁻¹³)
pH=12.72

I hope this helps. Let me know if anything is unclear.

7 0

3 years ago

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