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3 years ago

Mass of 4.50 moles of oxygen gas. Answer with 3 significant digits

Chemistry

1 answer:

goldfiish [28.3K]3 years ago

3 0

Answer:

The answer is 144g

Explanation:

This is because oxygen gas (O2) has a mass of 32g and you have 4.5 moles of O2, so you have to multiply 4.5 and 32.

You might be interested in

If 16.00 g of O₂ reacts with 80.00 g NO, how many grams of NO₂ are produced? (enter only the value, round to whole number)

Norma-Jean [14]

Answer:

46 g

Explanation:

The balanced equation of the reaction between O and NO is

2 NO + O₂ ⇔ 2 NO₂

Now, you need to find the limiting reagent. Find the moles of each reactant and divide the moles by the coefficient in the equation.

NO: (80 g)/(30.006 g/mol) = 2.666 mol

(2.666 mol)/2 = 1.333

O₂: (16 g)/(31.998 g/mol) = 0.500 mol

(0.500 mol)/1 = 0.500 mol

Since O₂ is smaller, this is the limiting reagent.

The amount of NO₂ produced will depend on the limiting reagent. You need to look at the equation to determine the ratio. For every mole of O₂ reacted, 2 moles of NO₂ are produced.

To find grams of NO₂ produced, multiply moles of O₂ by the ratio of NO₂ to O₂. Then, convert moles of NO₂ to find grams.

0.500 mol O₂ × (2 mol NO₂/1 mol O₂) = 1.000 mol NO₂

1.000 mol × 46.005 g/mol = 46.005 g

You will produce 46 g of NO₂.

6 0

3 years ago

The titration of 25.0 mL of an iron(II) solution required 18.0 mL of a 0.145 M solution of dichromate to reach the equivalence p

Svetlanka [38]

Answer:

0.64 M

Explanation:

Given:

Volume of iron(II) solution (V₁) = 25.0 mL = 0.025 L

Molarity of iron(II) solution (M₁) = ?

Number of moles of iron(II) solution (n₁) = ?

Volume of dichromate solution (V₂) = 18.0 mL = 0.018 L

Molarity of dichromate solution (M₂) = 0.145 M

Number of moles of dichromate solution (n₂) = ?

Molarity is equal to the ratio of moles and volume.

So, molarity of dichromate solution is given as:

$M_2=\frac{n_2}{V_2}\\\\n_2=M_2\times V_2=0.145\times 0.018 = 2.61\times 10^{-3}\ mol$

Now, let us write the complete balanced reaction for the given situation.

So, the complete balanced equation is given below.

$6Fe^{2+}(aq)+Cr_2O_7^{2-}(aq)+14H^+(aq)\to 6Fe^{3+}(aq)+2Cr^{3+}(aq)+7H_2O$

From the equation, it is clear that, 1 mole of dichromate is required for 6 moles of iron(II) solution.

So, using unitary method, we find the number of moles of iron(II) solution.

1 mole of dichromate = 6 moles of iron(II)

∴ n₂ moles of dichromate = 6n₂ moles of iron(II)

= $6\times 2.61\times 10^{-3}=0.016\ mol\ Fe^{2+}$

So, 0.016 moles of iron(II) is needed. Therefore, $n_1=0.016\ mol$

Now, molarity of iron(II) solution is given as:

Molarity = Moles ÷ Volume

$M_1=\frac{n_1}{V_1}\\\\M_1=\frac{0.016\ mol}{0.025\ L}=0.64\ M$

Therefore, the molarity of the iron(II) solution is 0.64 M.

4 0

3 years ago

The number of proton, neutrons and electrons in oxygen atom

Ksenya-84 [330]

Answer:

in an oxygen atom there are:

protons:8

electrons:8

neutrons:8

Explanation:

this is because the atomic number of oxygen is 8 and that is the proton number and the electron number is the same as the atomic number

4 0

3 years ago

Perform the following

Dmitry [639]

Answer:

0.5474

Explanation:

3.22 x 0.17

322 x 17 = 5,474

[] There are four places "after" the decimal in 3.22 and 0.17 combined, meaning we move the decimal to the right four times in our current answer

-> 5,474 becomes 0.5474

Have a nice day!

I hope this is what you are looking for, but if not - comment! I will edit and update my answer accordingly. (ノ^∇^)

- Heather

4 0

2 years ago

Water can be formed from the synthesis reaction of hydrogen with oxygen<br><br> PLEASE HELP

Anestetic [448]

Answer:

1.4 mols

4th answer

Explanation:

22. 5 g of O2 in moles = (22.5/32) mols = 0.703 mol

The stoichiometry between O2 and H2O =1: 2

Therefore H2O produced = 2 * 0.703 mols=1.406 mols

8 0

3 years ago