Is the cyanide ion a strong or weak base?

Which of the following best describes a safety precaution needed in nuclear power plants? (1 point)

kap26 [50]

Nuclear power plants produce energy in terms of electricity from radioactive materials. These elements are highly unstable due to their high neutron-to-proton ratio. That's why they spontaneously decay by giving off sub-atomic particles which yields a new element. So, nuclear reactions, fission and fusion, produce 'clean' energy because they do not produce gaseous by-products that could harm the environment. They only yield radioactive materials that could be harmful to the health of people nearby the area. Because of this risk, safety precautions are needed in a nuclear power plant.

Smokestacks are no longer used in nuclear power plants because there are no gases. So, the first choice is eliminated. Next, you should NOT ventilate the radioactive materials. Remember this radiation travels through all types of matter so it is harmful. These type of materials are strictly contained and handled. The third choice is correct because it prevents radiation to reach the outside environment. The last option, on the other hand, is not justifiable. Before a nuclear power plant is approved by the government, it is made sure that all its employees and employers are inherently safe. Otherwise, it would not be put into operation.

Therefore, the answer is letter C.

7 0

2 years ago

A given volume of gas at a temperature of 100 K has a

stepan [7]

Answer:

200K

Explanation:

Pressure is directly proportional to temperature.

100=225

x=450

(100*450)/225=x

x=45000/225

x=200

6 0

3 years ago

One mole of an ideal gas is sealed in a 22.4-L container at a pressure of 1 atm and a temperature of 273 K. The temperature is t

Ket [755]

Answer:

1.11 atm

(P, T)

2.83 atm

0.740 g

0.179 g/L, 0.158 g/L

N₂

Explanation:

One mole of an ideal gas is sealed in a 22.4-L container at a pressure of 1 atm and a temperature of 273 K. The temperature is then increased to 304 K, but the container does not expand. What will the new pressure be?

Assuming ideal behavior, we can calculate the new pressure (P₂) using Gay-Lussac's law.

$\frac{P_{1}}{T_{1}} =\frac{P_{2}}{T_{2}} \\P_{2}=\frac{P_{1}}{T_{1}}.T_{2}=\frac{1atm}{273K} .304K=1.11atm$

The most appropriate formula for solving this problem includes only which variables?

Gay-Lussac's law includes pressure (P) and absolute temperature (T).

Q2) A sample of nitrogen gas in a 1.69-L container exerts a pressure of 1.37 atm at 17 °C. What is the pressure if the volume of the container is maintained constant and the temperature is raised to 327 °C?

Initially the system is at 17°C (290 K) and the temperature is raised to 327°C (600 K). We can calculate the new pressure using Gay-Lussac's law.

$\frac{P_{1}}{T_{1}} =\frac{P_{2}}{T_{2}} \\P_{2}=\frac{P_{1}}{T_{1}}.T_{2}=\frac{1.37atm}{290K} .600K=2.83atm$

Q3) A gas mixture with a total pressure of 770 mmHg contains each of the following gases at the indicated partial pressures: 120 mmHg CO₂, 227mmHg Ar, and 190 mmHg O₂. The mixture also contains helium gas .

What mass of helium gas is present in a 14.0-L sample of this mixture at 282 K?

First, we have to calculate the pressure of Helium. We know that the total pressure is the sum of partial pressures.

Ptotal = pCO₂ + pAr + pO₂ + pHe

pHe = Ptotal - pCO₂ - pAr - pO₂

pHe = 770mmHg - 120mmHg - 227mmHg - 190mmHg=233mmHg

We can calculate the moles of Helium using the ideal gas equation.

$P.V=n.R.T\\n=\frac{P.V}{R.T} =\frac{233mmHg.14.0L}{(0.08206atm.L/mol.K).282K} .\frac{1atm}{760mmHg} =0.185mol$

The molar mass of He is 4.00g/mol.

$0.185mol.\frac{4.00g}{mol} =0.740g$

Calculate the density of oxygen, O₂, under each of the following conditions:

STP

1.00 atm and 35.0 ∘C

Express your answers numerically in grams per liter. Enter the density at STP first and separate your answers by a comma.

STP stands for Standard Temperature and Pressure. The standard temperature is 273 K and the standard pressure is 1 atm.

We can calculate the density using the following expression:

$\rho=\frac{P.M}{R.T} =\frac{1.00atm.4.00g/mol}{(0.08206atm.L/mol.K).273K} =0.179 g/L$

At 1.00 atm and 35.0 °C (308 K)

$\rho=\frac{P.M}{R.T} =\frac{1.00atm.4.00g/mol}{(0.08206atm.L/mol.K).308K} =0.158 g/L$

To identify a diatomic gas (X₂), a researcher carried out the following experiment: She weighed an empty 4.1-L bulb, then filled it with the gas at 2.00 atm and 24.0 ∘C and weighed it again. The difference in mass was 9.5 g . Identify the gas. Express your answer as a chemical formula.

We will look for the molar mass of the compound using the ideal gas equation.

$P.V=n.R.T=\frac{m}{M} .R.T\\M=\frac{m.R.T}{P.V} =\frac{9.5g \times (0.08206atm.L/mol.K)\times 297K }{2.00atm \times 4.1L} =28g/mol$

If the molar mass of X₂ is 28 g/mol, the molar mass of X is 14 g/mol. Then, X is nitrogen and X₂ is N₂.

5 0

3 years ago

A chef is serving a lunch special with 1 sandwich and 2 corn cobs per plate. If there are 5 sandwiches and 14 corn cobs, what is

shtirl [24]

5 plates is the highest amount that can be served

There’s only 5 sandwiches so 7 is automatically ruled out, there’s 14 corn cobs and 5 sandwiches only need 10 so it works out

7 0

3 years ago

Read 2 more answers

Burning gasoline as fuel for a car involves

Nostrana [21]

Thermal energy

mechanical energy

chemical energy

3 0

3 years ago

Read 2 more answers