Mechanical waves travel fastest through A -Solid B -Liquid C -Gas D -Vacuum

Gaseous methane (CH4) reacts with gaseous oxygen gas (O2) to produce gaseous carbon dioxide (CO2) and gaseous water (H2O) . If 0

UkoKoshka [18]

Answer: The percent yield of water is 84.72 %

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For methane:

Given mass of methane= 0.16 g

Molar mass of methane = 16 g/mol

Putting values in equation 1, we get:

$\text{Moles of methane}=\frac{0.16g}{16g/mol}=0.01mol$

For oxygen gas:

Given mass of oxygen gas = 0.25 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

$\text{Moles of oxygen gas}=\frac{0.25g}{32g/mol}=0.008mol$

The chemical equation for the reaction is

$CH_4+2O_2\rightarrow CO_2+2H_2O$

By Stoichiometry of the reaction:

2 moles of oxygen gas reacts with 1 mole of methane

So, 0.008 moles of oxygen gas will react with = $\frac{1}{2}\times 0.008=0.004mol$ of methane

As, given amount of methane is more than the required amount. So, it is considered as an excess reagent.

Thus, oxygen gas is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of oxygen gas produces = 2 moles of water

So, 0.008 moles of oxygen gas will produce = $\frac{2}{2}\times 0.008=0.008moles$ of water

Mass of water= $moles\times {\text{Molar Mass}}=0.008\times 18=0.144g$

To calculate the percentage yield of titanium (IV) chloride, we use the equation:

$\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

Experimental yield of water = 0.122

Theoretical yield of water = 0.144 g

Putting values in above equation, we get:

$\%\text{ yield of water}=\frac{0.122g}{0.144g}\times 100\\\\\% \text{yield of water}=84.72\%$

Hence, the percent yield of water is 84.72%.

7 0

3 years ago

What's mole in 34g of H2O

enyata [817]

Answer:

I hope you have the answer now

Explanation:

u an

3 0

3 years ago

Consider the following chemical reaction:

laiz [17]

Answer:

B. 1.65 L

Explanation:

Step 1: Write the balanced equation

2 SO₂(g) + O₂(g) ⇒ 2 SO₃(g)

Step 2: Calculate the moles of SO₂

The pressure of the gas is 1.20 atm and the temperature 25 °C (298 K). We can calculate the moles using the ideal gas equation.

P × V = n × R × T

n = P × V / R × T

n = 1.20 atm × 1.50 L / (0.0821 atm.L/mol.K) × 298 K = 0.0736 mol

Step 3: Calculate the moles of SO₃ produced

0.0736 mol SO₂ × 2 mol SO₃/2 mol SO₂ = 0.0736 mol SO₃

Step 4: Calculate the volume occupied by 0.0736 moles of SO₃ at STP

At STP, 1 mole of an ideal gas occupies 22.4 L.

0.0736 mol × 22.4 L/1 mol = 1.65 L

6 0

3 years ago

True or false atoms of difference elements can combine to form compound?

motikmotik

It's true

There are thousands of combinations that can be put together to form a all sorts of compounds. That's the whole basis of inorganic chemistry. Organic chemistry is a little bit different. It is more restricted.

3 0

3 years ago

Read 2 more answers

At what temperature a gas with volume 175 L at 15 oC and 760mmHg will occupy a volume of 198 L at a pressure 640mmHg?

MrRissso [65]

Answer:

To calculate the pressure when temperature and volume has changed, we use the equation given by combined gas law. The equation follows:

\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}

T

1

P

1

V

1

=

T

2

P

2

V

2

where,

P_1,V_1\text{ and }T_1P

1

,V

1

and T

1

are the initial pressure, volume and temperature of the gas

P_2,V_2\text{ and }T_2P

2

,V

2

and T

2

are the final pressure, volume and temperature of the gas

We are given:

\begin{gathered}P_1=760mmHg\\V_1=175L\\T_1=15^oC=[15+273]K=288K\\P_2=640mmHg\\V_2=198L\\T_2=?K\end{gathered}

P

1

=760mmHg

V

1

=175L

T

1

=15

o

C=[15+273]K=288K

P

2

=640mmHg

V

2

=198L

T

2

=?K

Putting values in above equation, we get:

\begin{gathered}\frac{760mmHg\times 175L}{288K}=\frac{640mmHg\times 198L}{T_2}\\\\T_2=274K\end{gathered}

288K

760mmHg×175L

=

T

2

640mmHg×198L

T

2

=274K

Hence, the temperature when the volume and pressure has changed is 274 K

7 0

3 years ago