All categories

1 year ago

Reference the following attachment

Chemistry

1 answer:

dem82 [27]1 year ago

3 0

The number of molecules of gases in each of the 3 vessels is the same.

<h3>Number of moles</h3>

The first vessel contains 2g of $H_2$ gas:

Number of molecules in 2 g = 2/2 = 1 mole

The second vessel contains 32 g of $O_2$ gas:

Number of molecules = 32/32 = 1 mole

The third vessel contains 44 g of $CO_2$ gas:

Number of molecules = 44/44 = 1 mole

Thus, the 3 vessels contain the same number of moles of gases.

More on the number of moles can be found here: brainly.com/question/12513822

#SPj1

You might be interested in

A gas with a volume of 20.0l at a pressure of 275 kpa is allowed to expand to a volume of 35.0l. what is the pressure in the con

sladkih [1.3K]

Answer:

$\boxed {\boxed {\sf 2. \ 157 \ kPa}}$

Explanation:

Since temperature remains constant, the only variables that change are volume and pressure. Therefore, we are using <u>Boyle's Law.</u> This states that the pressure is inversely proportional to the volume. The formula is:

$P_1V_1=P_2V_2$

We know the gas starts with a volume of 20.0 liters at a pressure of 275 kPa. We can substitute these values into the left side of the formula.

$275 \ kPa *20.0 \ L=P_2V_2$

We know the gas expands to a volume of 35.0 Liters, but we do not know the pressure.

$275 \ kPa *20.0 \ L=P_2* 35.0 \ L$

Since we are solving for the new pressure, we must isolate the variable P₂. It is being multiplied by 35.0 Liters and the inverse of multiplication is division. Divide both sides by 35.0 L.

$\frac {275 \ kPa * 20.0 \ L}{ 35.0 \ L}= \frac{P_2*35.0 \ L}{35.0 \ L}$

$\frac {275 \ kPa * 20.0 \ L}{ 35.0 \ L}=P_2$

The units of liters cancel.

$\frac {275 \ kPa * 20.0 }{ 35.0 }=P_2$

$\frac {5500}{35.0} \ kPa= P_2$

$157.142857 \ kPa=P_2$

The original measurements of pressure and volume have 3 significant figures, so our answer must have the same. For the number we calculated, that is the ones place.

The 1 in the tenths place (157.142857) tells us to leave the 7 in the ones place.

$157 \ kPa= P_2$

If the gas expanded to a volume of 35.0 liters while the temperature remained constant, the pressure in container was approximately 157 kilopascals.

8 0

2 years ago

In a constant-pressure calorimeter, 55.0 mL of 0.340 M Ba(OH), was added to 55.0 mL of 0.680 M HCI. The reaction caused the temp

Brut [27]

Answer:

Ba(OH)2 + 2 HCl → BaCl2 + 2 H2O

The reactants are present in equimolar amounts, so there is no excess or limiting reactants.

(0.0500 L) x (0.600 mol/L HCl) x (2 mol H2O / 2 mol HCl) = 0.0300 mol H2O

(4.184 J/g·°C) x (50.0 g + 50.0 g) x (25.82 - 21.73)°C = 1711.256 J

(1711.256 J) / (0.0300 mol H2O) = 57042 J/mol = 57.0 kJ/mol H2O

Explanation:

4 0

2 years ago

A sealed vessel containing sulfur dioxide and nitrogen has a total pressure of 520 Torr and partial pressures of 266 Torr nitrog

mixer [17]

The total pressure is the sum of all the partial pressures of the different components in the system. In this case, if the total pressure is 520 torr, and the partial pressure of nitrogen is 266 torr, and the only components are nitrogen and sulfur dioxide, this means that the rest of the pressure is all due to sulfur dioxide.
So the partial pressure of sulfur dioxide = 520 - 266 = 254 torr SO2.

8 0

3 years ago

X2O3 contain 32% of oxygen by mass , find the value of x.

denis-greek [22]

34g
Considering total mass as100g
I am sorry if it’s wrong

5 0

3 years ago

What is the mass in grams of 0.0015 mol of aspirin (C9H8O4)

almond37 [142]

Answer:

116.1 g

Explanation: