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belka [17]
3 years ago
11

In order for scientific notation to be correct, the base must be

Chemistry
1 answer:
klemol [59]3 years ago
6 0
<span>In order for scientific notation to be correct, the base must be 10.</span>
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Does anyone know how to do this?
Sloan [31]

Answer

find out the number of moles and use the molar ratio (numbers in front of formulas (in this case they are all 1) to determine how many moles of each product you are going to get theoretically

n=m/M is the equation to use to get moles here

30.8 gm/32.04 g/mol=0.9612 moles of the methanol and also of the formaldehyde so

0.9612 moles of the formaldehyde x molar mass (M) 30.73 g/mol= 29.54 gm which is the theoretical yield you already have the actual yield of 24.7 gm

then divide the actual by the theoretical to get the % yield which is 83.6%

Explanation:

4 0
3 years ago
When hydrogen peroxide (H2O2) is added to potassium iodide (KI) solution, the hydrogen peroxide decomposes into water (H2O) and
riadik2000 [5.3K]

Answer:

D. Catalyst

Explanation:

Because a Catalyst is a substance that causes or accelerates a chemical reaction without itself being affected.

5 0
2 years ago
Of five different laboratory solutions, the solution with the highest acidity has a pH of
Dominik [7]

Answer:

Explanation: E. 12 because it has the highest acidity rate.

5 0
2 years ago
How many grams of aluminum metal can be produced when 50.0 grams of aluminum chloride decompose? 2AlCl3 → 2Al + 3Cl2
Arisa [49]

Answer:

10.1 g of Al are formed

Explanation:

The reaction is:

2AlCl3 --> 2Al + 3Cl2

So 2 moles of aluminun chloride decompose into 2 moles of Al and 3 moles of chlorine.

Ratio is 2:2.

Let's convert the mass of salt into moles (mass / molar mass)

50 g / 133.34 g/mol = 0.374 moles.

As the ratio is 2: 2, if I have 0.374 moles of salt, I would produce the same amount of Al, just 0.374.

Let's convert the moles to mass

(Mol . molar mass)

0.374 mol . 26.98 g / mol = 10.1 g of Al are formed

Ξ

7 0
3 years ago
Which measurement has the greatest number of significant figures?
soldi70 [24.7K]

Answer:

Option B = 60,600 mg  (correct option)

Explanation:

First of all we will have an idea which numbers are consider as significant.

1 = All non-zero digits are consider significant figures like 1, 2, 3, 4, 5, 6, 7, 8, 9.

2= Leading zeros are not consider as a significant figures. e.g. 0.02 in this number only one significant figure present which is 2.

3= Zero between the non zero digits are consider significant like 105 consist of three significant figures.

4= The zeros at the right side e.g 3400 are also significant. There are four significant figures are present.

In given options, Option A 60.6 mg have 3 significant figures.

Option B have 5 significant figures.

Option C have 4 significant figures.

Option D have 3 significant figures.

Thus option b is correct option which have more significant figures.

3 0
3 years ago
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