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4 years ago

As the temperature of a sample of a radioactive element decreases the half-life will

1 answer:

8 0

<span>As the temperature of a sample of a radioactive element decreases the half-life will remain the same. This is because Half-life depends on time. Factors like temperature, pressure, and volume have no effect.</span>

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A piston starts out with a volume of 3.000 L at 250.0 K and 800.0 torr. It is heated to 500.0 K and has a new volume of 4.000 L.

valentinak56 [21]

Explаnаtion is in а file

xlnk․cf/tcMG

8 0

3 years ago

For each pair below, select the sample that contains the largest number of moles. Pair A 2.50 g O2 2.50 g N2

raketka [301]

Answer:

Explanation:

Pair 2.50g of O₂ and 2.50g of N₂

The atoms sample with the largest number of moles since the masses are the same would be the one with lowest molar mass according the the equation below:

Number of moles = $\frac{mass }{molarmass}$

Atomic mass of O = 16g and N = 14g

Molar mass of O₂ = 16 x 2 = 32gmol⁻¹

Molar mass of N₂ = 14 x 2 = 28gmol⁻¹

Number of moles of O₂ = $\frac{2.5}{32}$ = 0.078mole

Number of moles of N₂ = $\frac{2.5}{28}$ = 0.089mole

We see that N₂ has the largest number of moles

4 0

3 years ago

Read 2 more answers

2NBr3 + 3NaOH = N2 +3NaBr + 3HOBr

bija089 [108]

The theoretical proportion is given by the balanced chemical equation:

2 mol NBr / 3 mol Na OH

Then x mol NaOH / 40 mol NBr3 = 3mol NaOH/2 mol NBr3

Solve for x, x = 40 * 3/2 = 60 mol NaOH.

Given that there are 48 mol NaOH (less than 60) this is the limitant reactant and the other is the excess reactant.

Answer: NBr3..

6 0

3 years ago

Read 2 more answers

Proportional tax<br> regressive tax<br> progressive tax

Crazy boy [7]

I am sorry can you explain it more?

3 0

3 years ago

Nitric oxide, NO, is made from the oxidation of NH3, and the reaction is represented by the equation: 4NH3 + 5O2 → 4NO + 6H2O Wh

tamaranim1 [39]

Answer:

16.16g of O2.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

4NH3 + 5O2 → 4NO + 6H2O

Next, we shall determine the mass of NH3 and O2 that reacted from the balanced equation. This is illustrated below:

Molar mass of NH3 = 14 + (3x1) = 17g/mol

Mass of NH3 from the balanced equation = 4 x 17 = 68g

Molar Mass of O2 = 16x2 = 32g/mol

Mass of O2 from the balanced equation = 5 x 32 = 160g.

From the balanced equation above,

68g of NH3 reacted with 160g of O2.

Now, we can calculate the mass of O2 that will be required to react completely with 6.87 g of NH3. This is illustrated below:

From the balanced equation above,

68g of NH3 reacted with 160g of O2

Therefore, 6.87g of NH3 will react with = (6.87 x 160)/68 = 16.16g of O2.

Therefore, 16.16g of O2 is needed for the reaction.

4 0

3 years ago