Which base is the strongest for the given [H+]? 10-9 10-11 10-10 10-12

72.7%  is the percent by mass of oxygen in carbon dioxide. A percent is obtained by multiplying the result by 100.

One approach to show the concentration for an element within a compound or component in a combination is as a mass percentage. The mass percentage is computed by dividing the total weight of the combination by the mass of each component and multiplying the result by 100%. The mass percent is calculated by dividing the mass that contains the compound and solute by the mass for the element or solute.

Molar mass of oxygen = 32 g/mole

Molar mass of carbon dioxide = 44 g/mole

mass percentage of oxygen =(molar mass of oxygen/molar mass of carbon dioxide)×  100

=(32/44)×  100

=72.7%

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Answer : The percent by mass of oxygen in carbon dioxide is, 72.72%

Solution : Given,

Molar mass of oxygen = 16 g/mole

Molar mass of carbon dioxide = 44 g/mole

As we know that there are 2 atoms of oxygen and 1 atom of carbon present in the carbon dioxide.

So, the molar mass of oxygen, = 2 × 16 = 32 g/mole

Now we have to calculate the percent by mass of oxygen in carbon dioxide.

Now put all the given values in this expression, we get

Therefore, the percent by mass of oxygen in carbon dioxide is, 72.72%

Answer:

The correct answer is option 3.

Explanation:

Whenever there is a formation of bond between 2 atoms energy is released. This energy release is due to stability gained by the atoms after the formation of a bond that is why extra energy is released as a heat into surroundings. Exact process is occurring when 2 bromine atoms form bond to give molecule of bromine.

Whenever there is a dissociation of bond between 2 atoms energy is given. The energy provided externally so as to break the stable bond present between the atoms.

Answer:

Explanation:

To calculate the largest amount of nitrogen gas (N2) that could be produced when ammonia gas (NH3) and oxygen gas (O2) react, you need to consider the balanced chemical equation for the reaction:

4 NH3(g) + 5 O2(g) -> 4 N2(g) + 6 H2O(g)

From the balanced equation, you can see that 4 moles of NH3 produce 4 moles of N2.

Now, let's calculate the number of moles of NH3 and O2 you have:

Moles of NH3 = 4.0 grams / molar mass of NH3

Moles of O2 = 8.0 grams / molar mass of O2

The molar mass of NH3 (ammonia) is approximately 17.03 g/mol, and the molar mass of O2 (oxygen) is approximately 32.00 g/mol.

Moles of NH3 = 4.0 g / 17.03 g/mol ≈ 0.235 moles

Moles of O2 = 8.0 g / 32.00 g/mol ≈ 0.250 moles

Now, you need to determine the limiting reactant, which is the reactant that is completely consumed and limits the amount of product formed. To do this, compare the mole ratio from the balanced equation to the actual moles of NH3 and O2:

NH3 : O2 = 4 moles : 5 moles

Since you have fewer moles of NH3 (0.235 moles) than the required 0.25 moles based on the mole ratio, NH3 is the limiting reactant.

Now, calculate the moles of N2 produced using the mole ratio:

Moles of N2 = Moles of NH3 (since it's the limiting reactant)

Moles of N2 = 0.235 moles

Now, you can convert moles of N2 to grams:

Mass of N2 = Moles of N2 x Molar mass of N2

The molar mass of N2 (nitrogen gas) is approximately 28.02 g/mol.

Mass of N2 = 0.235 moles x 28.02 g/mol ≈ 6.59 grams

Rounding to the nearest gram, the largest amount of N2 that could be produced is approximately 7 grams.

The density of Argon gas at a pressure of 753 mmHg and a temperature of 35 °C is equal to 1.59 g/L.

What is the ideal gas equation?

The state of a quantity of gas is calculated by its pressure, volume, and temperature. The ideal gas law can be explained as the product of the volume and pressure of gas is equal to the multiplication of the universal gas constant and absolute temperature.

The mathematical equation for an ideal gas can be written as follows:

PV = nRT

PV =(m/M) RT

PM/RT = m/V

d = PM/RT

Where n is the moles of gas, T is the temperature of the gas,  V is the volume of the gas,  and R is the gas constant.

Given, the temperature of argon gas, T = 35 °C = 35 +273 = 308 K

The pressure of the argon gas, P = 753 mmHg = 1.01 atm

The molar mass of the Argon gas, M = 40 g/mol

Substitute  V, R, P, and T in the ideal gas equation, we get:

The density of Argon gas, d = PM/RT

d= 1.01 ×40/(0.082 × 308)

d = 1.59 g/L

Therefore, the density of Ar gas is 1.59 g/L.

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Answer:

Option (A)

Explanation:

Radioactivity is defined as a process in which an unstable atomic nucleus decays continuously and after a specific period of time changes into a much more stable element. During this time of decay, the nucleus emits charged particles (energy) which are known as the α, β and γ particles. These are often emitted in the form of electromagnetic energy and are very dangerous to health.

The radioactive elements decay at a certain rate which is commonly known as the half-life. Half-life is basically defined as the time required by a radioactive substance to decay half of its initial composition.

Thus, the correct answer is option (A).

Answer:

4

Explanation: