In order to draw a conclusion, scientists must______

What is the molar mass of lead nitrate (Pb(NO3)2) from the equation below?

AveGali [126]

Answer:

331.2 g/molExplanation:

3 0

3 years ago

Number of moles in 1.806*10^22 molecules of nitrogen

Fynjy0 [20]

Hi there!

• Avogadro's number = 6.023 × 10²³
• No.of molecules in N = 1.806 × 10²² [ Given ]

It's known that :-

Number of molecules = Moles × Avogadro's number

=> 1.806 × 10²² = Mol. × 6.023 × 10²³

=> Mole = $\dfrac {1.806 \cdot 10^{22} }{6.023 \cdot 10^{23} }$

=> Moles = 0.03 mol.

Hence, 0.03 mol. is th' required answer.

~ Hope it helps!

3 0

3 years ago

How do you solve this

denpristay [2]

Answer:

Explanation:

You simply have to multiply it by the molar mass =

m = 50mol SnSO4 x 214.773 g/mol

m = 10.738 g SnSO4

4 0

3 years ago

Read 2 more answers

A gas generation tube contains both the reactants involved in a chemical reaction and the gases that are produced.

Lady bird [3.3K]

The reaction will come to an end if all the reactants are used up. The reaction's limiting reactant is reactant B.

Limiting Reactant: The limiting reactant is the one that is consumed first and sets a limit on the quantity of product(s) that can be obtained.

This reactant is the one that restricts the production of products throughout the reaction. The reaction will come to an end if all of the reactants are used up.

surplus reactant

This is the limiting reactant that is present in excess and reacts with it all. Oxygen in the surroundings, as an illustration.

When all of the reactant B has been utilized, the reaction ends.

Learn more about limiting reactants here brainly.com/question/6751172

#SPJ4.

5 0

1 year ago

The masses of carbon and hydrogen in samples of four pure hydrocarbons are given above. The hydrocarbon in which sample has the

enot [183]

Answer:

Sample B

Explanation:

In this case, we need to determine the empirical formula for each sample. The one that match the formula of the propene would be the sample.

Let's do Sample A:

C: 60 g; H: 12 g

1. Calculate moles:

We need the atomic weights of carbon (12 g/mol) and hydrogen (1 g/mol):

C: 60 / 12 = 5

H: 12 / 1 = 12

2. Determine number of atoms in the formula

In this case, we just divide the lowest moles obtained in the previous part, by all the moles:

C: 5 / 5 = 1

H: 12 / 5 = 2.4 or rounded to two

3. Write the empirical formula:

Now, the prior results, represent the number of atoms in the empirical formula for each element, so, we put them with the symbol and the atoms as subscripted:

C₁H₂ = CH₂

Therefore, sample A is not the same as propene.

Sample B:

C: 72 g H: 12 g

Following the same steps, let's determine the empirical formula for this sample

C: 72 / 12 = 6 ---> 6 / 6 = 1

H: 12 / 1 = 12 ----> 12 / 6 = 2

EF: CH₂

Sample C:

C: 84 g H: 10 g

C: 84 / 12 = 7 ----> 7 / 7 = 1

H: 10 / 1 = 10 ----> 10 / 7 = 1.4 or just 1

EF: CH

Sample D

C: 90 g H: 10 g

C: 90 / 12 = 7.5 -----> 7.5 / 7.5 = 1

H: 10 / 1 = 10 -------> 10 / 7.5 = 1.33 or just 1

EF: CH

Neither compound has the same empirical formula as C3H6, but C3H6 is a molecular formula, so, if we just simplify the formula we have:

C3H6 -----> CH₂

Therefore, sample B is the one that match completely. Sample B would be the one.

Hope this helps

8 0

3 years ago

In order to draw a conclusion, scientists must_______ data from an investigation