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2 years ago

URGENT!

Chemistry

2 answers:

Law Incorporation [45]2 years ago

7 0

Answer:

Yea what they said^

Explanation:

Option 4 or D is correct

8.7 is your answer

MARK THE OTHER PERSON BRAINLIEST!!!

tensa zangetsu [6.8K]2 years ago

5 0

Answer:

Explanation:

A weak acid and a strong base will form a basic salt.

Option A is acidic, this pH would be found in salts formed from reactions between strong acids and weak bases.

B and C are neutral or close to neutral and as such will be formed from weak acids and weak bases, or strong acids and strong bases.

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Help please! -A compound contains 0.013 moles of carbon, 0.039 moles of hydrogen and 0.0065 moles of oxygen. Determine the empir

stepan [7]

A) C2H6O1

To find the emperical formula, divide each mole value by the smallest

For carbon, 0.013/0.0065 = 2

For hydrogen, 0.038/0.0065= 6

For oxygen, 0.0065/0.0065= 1

Emperical formula = C2H6O1

8 0

2 years ago

Read 2 more answers

NEED HELP FAST!!

koban [17]

Answer:

I'm pretty sure that's right.

Explanation:

Download pdf

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2 years ago

What is the name of KMnO3???

bonufazy [111]

The answer is potassium magnate

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2 years ago

In the reaction, A → Products, the rate constant is 3.6 × 10−4 s−1. If the initial concentration of A is 0.548 M, what will be t

Arada [10]

Answer:

$\large\boxed{\large\boxed{0.529M}}$

Explanation:

Since the rate constant has units of s⁻¹, you can tell that the order of the reaction is 1.

Hence, the rate law is:

$r=d[A]/dt=-k[A]$

Solving that differential equation yields to the well known equation for the rates of a first order chemical reaction:

$[A]=[A]_0e^{-kt}$

You know [A]₀, k, and t, thus you can calculate [A].

$[A]=0.548M\times e^{-3.6\cdot 10^{-4}/s\times99.2s}$

$[A]=0.529M$

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2 years ago

Why are metal containers not used for storing acids

kaheart [24]

Answer : Metal containers are not used for storing acid because most of the time acid reacts with almost every metal and produces salts or oxides which alters the acid characteristics making it useless .......

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2 years ago